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1
CHAPTER –I
RATE OF CHEMICAL REACTION AND CHEMICAL EQUILIGBRIUM
1. Which of the following reactions are slow and which are the fast?
i) Setting of cement.
ii) Formation of coal in the earth crust.
iii) Reaction between aqueous solution BaCl2 and H2SO4.
Ans.
(i)
(ii)
(iii)
Setting of Cement.
Formation of coal.
Rect. Bet. (Aq) BaCl2 & H2SO4.
Fast reaction.
slow reaction.
Fast reaction.
2. Give one example in case of a reaction, which takes place
i) Instantaneously.
ii) At moderate rate.
Ans.
(i) Instantaneously
a. Silver nitrate + sod. Chloride
silver Chloride + sod. Nitrate
AgNO3(aq) + NaCl(aq)
AgCl(s) + NaNO3(aq)
b. Barium Chloride + Hydrogen Sulphate
BaCl2(aq)
c.
2Mg
+
+
Barium sulphate + Sodium Chloride.
H2SO4
BaSO4(s)
O2
+
2HCl(aq)
2MgO
ii) Moderate.
a.CH3COOH (aq)
+ C2H5OH(aq)
H2SO4
CH3COOC2H5
+ H2O
MnO2
b.2KClO3
2KCl
+
3O2
3. How will you define the rate of a chemical reaction? What is the
meaning of average rate of chemical reaction?
Ans.
The rate of disappearance of a reactant or reactants
(OR)
2
The rate of appearance of a product or products
(OR)
Rate of reaction = Change in conc. Of a reactants or products
Time taken
Eg: NO2(g)
+ CO(g)
Rate of reaction =
-Δ[NO2]
Δt
CO2(g)
=
-Δ[CO]
Δt
+
NO(g)
= Δ[CO2]
Δt
= Δ[NO]
Δt
4. What are various factors, which affect the rate of a chemical reaction?
Explain with the suitable examples.
Ans;
The rate of a reaction depends upon the following factors
a) Concentration of the reactants.
b) Effect of Temperature.
c) Effect of Catalyst.
d) Effect of Light/radiation.
e) Surface area of the reactants.
a) Concentration of the reactants:
The rate of a reaction generally increases with increase in
Concentration of reactant of reactants.
For example in 2NO+O2-->2NO2 reaction, the reaction rate doubles when O2
concentration doubles.
The rate of reaction quadruples when “NO” concentration doubles.
(b) Effect of Catalyst:
Catalysts are substances, which alters the rate of chemical reactions with
out undergoing any significant change.
If the catalyst increases the rate of reaction it is named as positive
catalysts.
Fe
N2+3H2
2NH3
Fe is +ve catalyst
NO
2SO2+O2
2SO3
NO is +ve catalyst
If the catalyst decreases/retards the rate of reaction it is named as
negative catalyst.
Glycerol
Eg:
2H2O2
2H2O + O2
Glycerol is –ve catalyst
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C) Effect of Light/Radiation
Rates of some reactions are influenced by light.
For example
photosynthesis, photography.
Blue printing such type of reactions are
called photochemical reactions.
Light
6CO2 + 6H2O
C6H12O6
Light
2 AgBr
2Ag + Br2
Light
H2 + Cl2
2HCl
d) Effect of Temperature:
The rate of the reaction increases with increase of temperature.
Perishable foods like milk, cooked vegetables go bad much more rapidly in
summer than in winter.
In the case of enzyme catalyzed reaction rate of reaction increases with
in creases of temperature at first up to a certain optimum temperature and
then rate of reaction decreases with increase of temperature.
f) Surface area of the reactants:
The rate of the reaction increases with increase in surface area of the
reactants. The smaller the size of reactant particles the greater is the
total surface area exposed for reaction and consequently greater is the
rate of the reaction.
For Eg:
Zn + 2HCl
ZnCl2 + H2↑
fast
(dust)
Zn
+ 2HCl
(Granules)
ZnCl2 + H2↑
5. What is the role of a catalyst in a reaction? Does catalyst undergo any
change at the end of a chemical reaction?
Ans.
A catalyst is a substance, which alters the rate of a chemical reaction.
A catalyst may increase or decrease the rate of a reaction.
Fe/Mo
+ 3H2
2NH3
Eg:
N2
(Catalyst)
Fe/Mo increases the rate of reaction. So Fe/Mo is called +ve catalyst.
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Glycerol
2H2O2
2H2 O
+
O2
(Catalyst)
Glycerol decreases the rate of reaction. So glycerol is –ve catalyst.
No, Catalyst doesn’t undergo any change chemically. A Catalyst may be
recovered in mass and composition at the end of the chemical reaction.
6. What is the effect of temperature on the following?
i) Dissociation of an electrolyte (dissolution is taken as an
endothermic process).
ii) Rate of a reaction in gaseous state.
iii) Concentration of product(s) of an exothermic reversible reaction
carried out in a closed container.
Ans.
i)Increases.
ii) Increases.
Iii) Decreases.
7. What do you mean by dynamic equilibrium? In what way is it different
from static equilibrium? Explain with suitable examples.
Ans.
In a reaction at the equilibrium the rate of forward reaction is
equal to the rate of backward reaction. In other words forward and back
word reaction continues even after equilibrium is reached. So equilibrium
is dynamic.
N2(g) + 3H2(g)
2NH3(g)
8. Can we achieve equilibrium between water and its vapour in an open
container? Explain your answer and say what will happen eventually?
Ans.
No; we can’t achieve equilibrium between water and its vapour in an
open
container.
Water vapour escapes into atmosphere.
9. Which of the following processes will be at equilibrium?
i) Water maintained at 233K in a closed container.
ii) Sulpher dioxide being released in atmosphere at 298K.
iii) Heating of calcium carbonate at 773K in a closed kiln.
Ans.
H2O(g)
At Equilibrium
i)
H2O(l)
5
(Liquid water )
ii)
2SO2
iii)
CaCO3
(Water vapour)
+ O2
2 SO2
CaO
+
CO2
At Equilibrium
10.Which of the following reactions will favour the formation of
product(s)
when the temperature is raised by 100C and reaction is carried out in a
closed container
i) N2(g) + 3H2(g)
2NH3(g)+ 92KJ
ii) 2Cl2(g) + 2H2O(g)
4HCl(g) + O2(g)
-113KJ
Ans
(i) N2(g) + 3H2(g)
2NH3(g) + 92KJ
The reaction is carried in closed container means reactant and products
are in dynamic equilibrium.
On increasing the temperature the equilibrium shifts towards
(exothermic side) left and ammonia will decompose to give N2 and H2.
(OR)
Equilibrium shifts back (Left side)
ii) 2Cl2(g) + 2H2O(g)
4HCl(g) + O2(g) -113KJ
As the reaction is carried out in closed container, it is in equilibrium.
On increasing the temperature the equilibrium shifts towards right.
11. Write the equilibrium constant for the following reactions
i)
ii)
iii)
iv)
Ans.
2NO2(9)
N2O4(g)
2SO2(g) + O2(g)
CO(g)+ 3H2(g)
Fe3+ (aq) + SCN(aq)
2SO3(g)
CH4(g) +H2O(g)
FeSCN2+(aq)
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(i)
2NO2(g)
N2O4(g)
ERROR
(ii) 2SO2(g) + O2(g)
2SO3(g)
(iii) CO(g)+ 3H2(g)
KC =
[N2O4]
[NO2]2
KC =
[SO3]2
[SO2]2[o2]
CH4(g) +H2O(g)
[CH4]+[H2O]
[CO][H2]3
(iv) Fe3+ (aq) + SCN-(aq)
KC
KC =
FeSCN2+(aq)
= [FeSCN2+]
[Fe3+][SCN-]
12. Classify the following acids and cases in the categories of weak and
strong
i) HCl
ii) H2SO4
iii) CH3COOH
iv) HCN
v) HClO4
vi) H3PO4
vii) NaOH
viii) Ca(OH)2
ix) NH4OH
Ans.
Strong acids:
HCl, H2SO4 ,HClO4 .
Weak acids: CH3COOH, HCN,H3PO4
Strong bases: NaOH
Weak bases: NH4OH, Ca(OH)2
13.Find the PH of the solutions if the acids are fully dissociated.
i)0.01M Hcl
ii)o.o5M H2SO4
Ans:
i) 0.01M Hcl.
+
ClHCl
H+
0.01M
[H+]
PH
P
0.01M
=
=
=
=
=
0.01M
1/100 M
10-2M
- log [H+]
-log [10-2]
7
=
=
=
-(-2log 10)
-(-2)
2.00
ii) 0.05M H2SO4
H2SO4
(0.05M)
[H+]
PH
P
=
=
=
=
=
=
=
=
2H+
(0.10M)
+
SO42-
0.10M
1/10 M
10-1M
-log [H+]
-log [10-1]
-1(-1 log10)
-1(-1)
1.00
14. Classify the following into strong and weak electrolytes on the basis
of their behaviour in aqueous solution.
I)
ii)
iii)
iV)
V)
NaCl
NH4 Cl
CH3COOH
HCN
NaOH
Ans.
Strong electrolytes
NaCl
NH4Cl
NaOH
Weak electrolytes
CH3COOH
HCN
15. Calculate the PH of the solution when hydrogen ion concentration is
i) 1.0x10-7M
ii) 1.0x10-9M
Ans.
PH
P
= -log [H+]
=-log [1.0x10-7]
=-log [log10-7]
=7log10
=7[1.0000]
=7.00
8
PH
= -log [H+]
= -log [1.0x10-9]
= -log [10-9]
= 9[1.0000]
= 9.00
16. At 298M equilibrium concentrations of the reactions and products for
the reaction H2 (g) + I2(g)
2HI(g) are as follows:
[HI] = 0.490M. [H2] =0.080M and [I2] = 0.060M Calculate the equilibrium
constant at this temperature
Ans.
P
H2(g) + I2(g)
2HI(g)
[H2]=0.080M;
[I2]=0.060M;
[HI]=0.490M.
[HI]2
KC
=
[0.49M]2
=
[H2] [I2]
0.2401
=
[0.080M][0.060M]
=50
0.0048
17. Equlibrium constants for the reactions given below are provided in the
right hand side at 298K.
2NO2(g)
KC=4.66x10-3
(i) N2O4(g)
(ii) 2NH3
Ans.
N2(g) +3H2(g)
KC= 3.0x10-9
In which case, formation of the products will be more favoured?
KC is directly proportional to the conc. of products. So the reaction in
which Kc value is more will be favorable for the formation of more
products.
2NO2(g)
KC=4.66x10-3
(i) N2O4(g)
(ii) 2NH3
N2(g) +3H2(g)
KC= 3.0x10-9
of first reaction (4.66x10-3) is more than the KC of second reaction.
KC
Hence, the Product formation will be more favoured in the case of first
reaction
2NO2(g)
N2O4(g)
9
CHAPTER-2
SOME IMPORTANT CHEMICAL COMPOUNDS
1. Give the Names of Raw Materials that are required for the manufacture
of
washing soda by solvay process. Write the reactions involved in the
process.
Common salt
Ammonia
Lime Stone
H2O
+ NH3
:
:
:
Ans:
NaCl.Sodium chloride.
NH3 .Ammonia
CaCO3.Lime stone (Calcium carbonate)
+ NaCl + CO2
NaHCO3 +
NH4Cl
Heat
Na2CO3+ CO2+H2O
2NaHCO3
Heat
CaCO3
CO2+CaO
CaO + H2O
Ca(OH)2+ 2NH4Cl
Ca (OH)2
CaCl2 +2NH3+2H2O
2. What is efflorescence? Name one compound which shows efflorescence?
support your answer with reaction?
Ans:
The processes of loosing water of crystallization, when the
substance is exposed to air for long time to form anhydrous or monohydric
substance is called as efflorescence.
Na2CO3 10 H2O, Sodium carbonate deca hydrate is one example.
10
Na2CO3 10 H2O
Na2CO3 H2O + 9H2O
3. State the important properties of washing soda.
Ans:
PHYSICAL PROPERTIES:
Washing soda is a transparent crystalline solid.
Washing soda is soluble in water.
Washing soda solution in water is alkaline which turns red litmus blue.
Washing soda is good cleansing agent which even works well with hard
water.
Washing soda shows Efflorescence.
CHEMICAL PROPERTIES:
1) Action of heat:
Heat
Na2CO3 1OH2O
Na2 CO3 + 10H2O
2) Action with dil. HCl
Na2CO3 + 2HCl
2NaCl + CO2 + H2O
3) Action with CO2
Na2CO3+SiO2
Na2SiO3+CO2
Sod. Silicate (soft glass)
4.What is the common name of Na2Co3. 10H2O? Name a metal carbonate which
is soluble in water.
Ans:
Common name of Na2CO3.10H2O is Washing soda.
Metal carbonate Soluble in
water is sodium carbonate or soda ash Na2CO3
5. Give important uses of washing Soda?
Ans:
Washing soda is used as cleaning agent in laundry and for domestic
purpose.
Washing soda is used for softening hard water
Washing soda is used in the manufacture of borax, glass,soap etc.
Washing soda is used as laboratory reagent in qualitative and quantitative
11
analysis.
6. Give important properties of baking soda
Ans:
PHSICAL PROPERTIES:
1. Baking soda is white in color.
2. Baking Soda is sparingly soluble in water.
3. Baking soda solution with water is alkaline and turns red litmus to
blue.
CHEMICAL PROPERTIES
Action of heat:
Baking soda gives CO2 on heating
Heat
2NaHCO3
Na2CO3+ H2O +CO2
Action of dil. Hcl
HCl + NaHCO3
NaCl
+ CO2 + H2O
7. A baker found that the cake prepared by him is hard and small in size.
Which ingredient has he forgotten to add that would have made the cake
Fluffy? Give reason.
Ans:
Baker forgotten to add NaHCO3, Baking soda.
NaHCO3 in the form of baking powder is added to dough for preparing cake
or bread. NaHCO3 on heating with food material decomposes to form CO2 due
to which cake or bread becomes light, fluffy and big in size.
2NaHCO3
Na2CO3
+
CO2 + H2O
8. Name the substance obtained by the action of chlorine on dry slaked
lime write chemical equation of the reaction.
Ans:
Calcium oxychloride (Bleaching Powder) is obtained by the action of
Chlorine gas,Cl2 on dry slaked lime Ca(OH)2.
Ca(OH)2 + Cl2
CaOCl2 + H2O
(Slaked lime)
(Bleaching powder)
9. How is bleaching powder prepared? Give the reaction?
Ans:
Bleaching Powder is prepared by passing chlorine gas over dry slaked lime.
Ca(OH)2 + Cl2
CaOCl2
+
H2O
12
10. What happens when beaching powder is exposed to air?
Ans:
Bleaching powder deteriorates giving off chlorine gas (Cl2) due to the
reaction with carbondioxide gas present in air CO2
CaOCl2 + CO2
CaCO3 + Cl2
11. What are the important uses of bleaching powder?
Ans:
It is used for disinfecting drinking of water.
It is used for bleaching cotton in textile industry.
It is used for bleaching wood pulp in paper industry.
It is used for the manufacture of chloroform,CHCl3
It is used as an oxidizing agent in chemical industries and laboratory.
12. Name the compound which is used in hospitals for setting fractured
Bones. Write its chemical name and formula. How is it prepared?
Ans:
is used in
Plaster of Paris (Calciumsulphate hemi hydrate) CaSO4 ½ H2O
hospitals for setting fractured bones.
Calcium sulphate hemi hydrate,CaSO4 ½ H2O
It is prepared by heating Gypsum at 373k (1000 C)
1000C
CaSO4 ½ H2O + 3/2 H2O
CaSO4 2H2O
13. What is gypsum? What happens when gypsum is heated to 373K?
Ans:
Calcium sulphate dehydrate is called as Gypsum.
CaSO4 2H2O is Gypsum
1000c
CaSO4 2H2O
CaSO4 ½ H2O + 3/2 H2O
373 k
Gypsum on heating at 373k forms plaster of Paris, CaSO4 ½ H2O
14. Give chemical equation for the preparation of lime?
ANS:
CaCO3
Heat
CaO
(s)
+
CO2
(g)
13
(Lime)
Calcium carbonate (Lime Stone) on heating in a lime kiln forms lime.
15. Give important uses of plaster of Paris?
Ans:
It is used in making toys, decorative material, jewellery, cosmetics and
casts for statues.
It is used for setting fractured bones in the right position.
It is used for sealing the air gaps in apparatus to make it air tight.
It is used for making smooth surfaces and ornamental designs.
16. How is slaked lime obtained from lime?
Ans:
Lime (Cao) reacts with water to form slaked lime Ca(OH)2
CaO + H2O
Ca(OH)2+ Heat
17. What happens when lime stone is heated strongly? Write the chemical
equation.
Ans:
Lime stone is calcium carbonate CaCo3, it decomposes to form quick lime Cao
and CO2 on heating.
CaCO3
(Lime Stone)
CaO
+
(quick lime)
CO2
18. A white powdered solid, when added to water produces a hissing sound.
Identify the compound. How this compound does reacts with moist hydrogen
chloride gas? Write the chemical equation. Give two uses of the same
compound.
Ans:
White powdered salt that produces hissing sound is lime CaO.(Calcium
oxide)
Ca(OH)2+Heat
CaO + H2O
It reacts with moist HCl to form CaCl2 and water.
CaO + 2HCl
CaCl2+H2O
Uses of CaO
i) CaO is used in manufacture of glass, cement, etc.,
ii) Cao is used as basic lining in furnaces.
iii) Cao is used for white washing.
iv) CaO is used in manufacture of bleaching powder.
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19. How is Cement manufactured?
Ans:
The raw materials used for the manufacture of cement are
i) Lime Stone (to provide CaO)
ii) Clay(to provide Al2O3, SiO2, Fe2O3)
The raw materials lime stone and clay are finely powdered and then
mixed togather in the ratio 3:1 by mass. This mixture is made into
homogenous by wet or dry processes. The finely Homogenized mixture of
clay and lime stone is heated in a rotary kiln to produce CLINKER.
The clinker is made in to fine powder and 2to5% gypsum is added to
regulate the setting time.
Diag: Ref.page number 20 fig.number2.4
20. Give some important uses of cement.
Ans: For making
1. Mortar:Cement is mixed with sand and required amount of water. This mixture is
called as mortar, which is used for plastering and binding bricks and
stones.
2. For making Concrete:It is a mixture of cement, gravel sand and water, which is used in
construction of buildings, dams, roads etc.,
3. For making Reinforced concrete cement:
Steel rods or steel frames are embedded in concrete, which useful in
construction of dams, buildings, and bridges.
21. What are the raw materials used for making glass?
Ans:
Sodium carbonate (soda ash) Na2CO3
Lime Stone (Calcium Carbonate) CaCO3
Sand (Silica, Silicon dioxide) SiO2
Broken Glass pieces (Cullet)
22. Describe the process of manufacture of ordinary glass?
Ans:
Raw Materials: soda ash (Sodium Carbonate, Na2Co3)
Lime Stone (Calcium Carbonate, CaCo3)
Silica (Silicon dioxide SiO2)
Cullet (Broken Glass)
The powdered raw materials soda ash, lime stone, silica is known as batch,
broken glasses are add to the raw materials and then heated to 14000C
(1673K) in the furnace. Cullet lowers the melting point of the batch.
The following chemical reactions takes place to form molten glass, over
molten glass scum is formed. The scum is skimmed off.
15
Na2CO3+SiO2
Na2SiO3 + CO2
CaCO3 + SiO2
CaSiO3 + CO2
The molten mixture of Na2SiO3 and CaSiO3 forms Solid glass on Cooling.
Na2SiO3+CaSiO3 + n SiO2
Na2SiO3. CaSiO3
nSiO2
(Glass)
23. How does Pyrex glass differ from soda glass?
Ans:
Soda Glass
01.It doesn’t contain boron and
Aluminum oxides.
02. It is prepared by fusing Na2CO3,
CaCo3
03. It is called Soft Glass because
it softens easily on heating.
04.It is easily attacked by
chemicals
05.It has high coefficient Of
expansion so it is unfit for
making laboratory apparatus
06.It is brittle and breaks easily
Pyrex Glass
01.It Contains boron and aluminum
oxides also
o2.It is prepared by fusing
Na2CO3,K2CO3,CaCO3,SiO2, AlO3and
borax.
03.It is very difficult to soften
Pyrex glass by heating
04.It is more resistant to chemicals
05.It has low coefficient of
expansion so it is used for
making laboratory apparatus
06.It is hard
24. What do you mean by annealing of glass?
Ans:
The process of cooling finished glass article very slowly and uniformly is
called annealing.
The annealing is so slow it will take sever days for
completion. Annealing prevents brittleness in glass
25. What are the applications of photo chromatic glasses?
Ans:
1. Photo chromatic glasses are used as sunshield glasses.
2. Photo chromatic glasses are used for making spectacles, goggles
and
cameras.
16
26. What are the different kinds of glasses? Mention their uses.
Ans:
Soda Glass(or soft glass)
Uses: for making
*
*
*
*
*
*
Glasses tumblers.
Dishes.
Bottles.
Mirrors.
Window panes.
Bulbs etc.
Hard Glass (or Potash Glass)
Uses: For making * hard glass laboratory apparatus.
* Glass bottles in which acids and bases are to be
preserved.
Lead Crystal Glass
Uses: For making
* Expensive Glassware.
* Decoration pieces.
* Cut glass articles.
27. How is steel manufactured by Bessemer process?
Ans: For fig ref.page number 22 fig.number2.6.
Steel is manufactured from pig iron in a Bessemer converter,
which is a pear shaped furnace lined inside with silicon. Molten pig iron
is taken in Bessemer converter is heated with a hot blast of air. Oxygen
present in the hot air reacts with impurities like Mn, Si, C, P to form
oxides some of these oxides escape into atmosphere and rest forms slag.
This slag is skimmed off. When all the impurities are removed, required
amount of carbon is added to molten iron to form steel of our choice.
The following reactions take place in Bessemer converter.
2Mn + O2
2MnO
Si + O2
SiO2
2C + O2
2CO
4P + 5O2
2P2O5
3CaO+ P2O5
Ca3(PO4)2 slag
MnO +SiO2
MnSiO3
slag
CaO +SiO2
CaSiO3
slag
28.Give important properties of Steel?
Ans:
Properties of steel depends on percentage of steel Iron containing
0.1
17
to 0.4 percent of carbon is mild steel
* Quite malleable.
* Ductile
* Elastic
* Very tough
* Not brittle
Iron containing 0.5 to 1.5 percent of carbon is hard steel
* Very hard
* Brittle
* High elasticity
29. What are the important uses of steel?
Ans:
01. Steel with 7 to 20% Manganese is very hard and tough used for
Helmets, Rock crushing machinery.
02. Chromium and nickel steel is used for making a aeroplane parts, motor
cars, bicycle, parts, radio valves, bulbs.
03. Cobalt steel is used for making permanent magnets.
04. Silica steel is used for making pipes and pumps which carry acids.
05.Tungsten chromium vanadium steel used or making drilling tools.
06.Stainless steel is used for making utensils surgical instruments etc.
18
CHAPTER 13
Metal and Non Metals
1. What are metals?
Metals are the elements (except Hydrogen) which form positive ions by
losing electrons. (Or)
Metals are the elements (except hydrogen) which form positive ions by
losing electrons and posses good electrical conductivity metals and
ductile
Example:
Na
Mg
Na+ + 1eMg2+ + 2e-
2. Explain why the surface of some metals acquires, a dull appearance
when exposed to air for a long time?
Metals react with oxygen, hydrogen sulphide, and carbon dioxide to
form metal oxide, metal sulphide and metal carbonates. So metals
acquire dull appearance which exposed to air for longtime.
For eg:
(O2)
CO2
Na
Na2O
Na2CO3
(air)
H2S
2Ag
Ag2S
(air)
19
3. What are amphoteric oxides? Give examples of two amphoteric oxides.
Metal oxides which show both acidic, as well as basic in nature are
amphoteric.
Eg:Al2O3 Aluminum Oxide
Zno
Zinc Oxide
4. Name two metals which do not react with oxygen.
Ag – silver.
Au – gold.
Pt – Platinum.
5. Which gas is produced when a metal reacts with dilute hydrochloric
acid? Write the chemical reaction when iron reacts with dil. H2SO4
Hydrogen gas is produced.
Fe(s) + H2SO4(aq)
FeSO4(aq) + H2(g)
6. Name two metals which can form hydrides with hydrogen.
Na – Sodium
Ca – Calcium
2Na(s) + H2(g)
Ca(s) + H2(g)
2NaH(s)
CaH2(s)
(sodium hydride)
(Calcium hydride)
7. What would you observe when zinc is added to a solution of iron(II)
sulphate? Write the chemical reaction that takes place.
Observations
(i)Pale green colour of the solution slowly changes to colourless.
ii)Iron is formed slowly at the bottom of the reaction vessel.
Zn(s) +
FeSO4(aq)
ZnSO4(aq)
+
Fe(s)
(Pale green)
(Colorless)
8. Describe briefly the froth flotation process for the concentration of
sulphide ores.
Fig: Ref. Page NO 170 of X std science and technology textbook
fig No: 14.2.
This forth floatation process is used to separate the gangue from
sulphide ores in which ore particles are lighter and gangue particles
are heavier.
Powdered ore particles, pine oil and water mixture is mechanically
agitated by blowing air with high pressure as shown in the above
figure. Forth formed in this process rises up with lighter sulphide
ore particles.
This forth is skimmed off which gives are particles
and heavier gang particles shinks to bottom of the tank.
20
9. Define the term metallurgy.
The extraction of metals from their ores and then refining the metal
for their use is known as metallurgy.
10.
Does every mineral have a definite and fixed composition? Explain.
No, Every mineral doesn’t have a definite and fixed composition.
Some minerals may contain a large percentage of metal where as
others
may contain only a small percentage of metal.
Some minerals may contain objectionable imparities which may hamper
the extractions of metals.
The mineral which has high percentage of metal and very less
objectionable impurities is known as ore from which metals are
extracted Profitably.
11.
What is bauxite? What are the main impurities that are found in this
ore? Briefly describe how the ore is purified.
Al2O3, Bauxite is the ore of Aluminum. Impurities are sand and iron
Oxide.
Purification: Bauxite is purified by Bayer’s process.In this
Process powdered ore is treated with aq. NaOH solution. Iron (III)
oxide and sand do not dissolve in sodium hydroxide solution. So
they
are separated by filtration. Al2O3 reacts with NaOHaq to form sodium
aluminate. Sodium aluminate converted into aluminum hydroxide
Al(OH)3
Which on heating produces Alumina Al2O3?
12.
NaOH(aq)
H2O
X
Al2O3
NaAlO2
Al (OH)3
Impure
sod.aluminate
Differentiate between roasting and calcination.
Al2O3
pure
i) In calcination the ore is heated in the absence of air where as
In roasting ore is heated in the presence of air.
ii) calcination is done for carbonate ores where as
Roasting is done for sulphide ores
13.
What is a Thermit reaction?
Highly reactive metals like aluminum Al can be used as reducing
agent
to reduce manganese dioxide MnO2, and Iron(III) oxide into Mn and Fe.
This reaction is called as thermite reaction.
3MnO2(s) +4Al(s)
3Mn(s) + 2Al2O3(s)
Fe2O3(s) +2Al
2Fe(s) + Al2O3(s)
[OR]
Al
Mn
MnO2
Heat
21
Al
Fe2O3
Fe
Heat
14.
Name the various processes used for refining of metals.
method
is used for refining volatile metals?
Which
i.
Liquation Method
ii.
Distillation Method
iii.
Electrolytic refining
Distillation method is used for refining volatile metals like
mercury
and zinc.
15.
Name two metals which will displace hydrogen from dilute acids, and
two metals which will not displace.
Metals which displace hydrogen from dilute acids are
Na-Sodium
Mg-Magnesium
Zn-Zinc
Fe-Iron
Metals which do not displace Hydrogen are
Cu –Copper
Au –Gold
Ag –Silver
16.
In the electrolytic refining of a metal M, name the anode, cathode
and the electrolyte.
M is aluminum
Anode
:
Cathode
:
Electrolyte
:
17.
Graphite rods
Graphite lining
Na3AlF6 Cryolyte.
What are the different functions of cryolite in the extraction of
aluminum by electrolytic reduction of alumina?
1. To lower the melting point of Alumina
2. To act as electrolyte
18.
What type of solution-acidic, basic or neutral, is formed by
dissolving the oxides of Group 1 in water?
Basic (alkaline)
19.
What important properties of aluminum are responsible for its great
demand in industry?
1.
2.
3.
4.
5.
High electrical conductivity,
High malleability
High ductility
High resistance to corrosion
Light in weight
22
20.
Draw the cell for the electrolytic reduction of alumina?
the anodes be replaced from time to time?
Why must
Ref Page No; 174; fig 14.5
Oxygen gas is liberated at anode, which reacts with graphite (carbon)
of anode to form CO2 gas, due to which graphite anode is to be
replaced.
C
+
(Carbon at anode)
21.
O2
(Oxygen lib.at anode)
CO2
carbon dioxide
Name the raw materials required for extracting iron.
1. hematite Fe2O3 or magnetite Fe3O4
2. Lime stone CaCO3
3. Coke
22.
Write the chemical reactions that take place in the blast furnace
for the extraction of iron from hematite.
C(s) + O2(g)
CO2(g) + Heat
CaCO3(s)
CaO(s) + CO2(g)
CaO + SiO2
CaSiO3(slag)
Fe2O3(s) +3CO(g)
23.
2Fe(a) + 3Co2(g)
Why is iron more useful when it is mixed with a little carbon?
When small amount of carbon 0.1 to 1.5 percent added to pure Iron it
forms an alloy called steel it is 1) Hard 2) strong 3)Less Rusting.
24.
What is the difference between pig iron and steel?
Pig Iron(cast Iron):- Pig Iron contains about 4 percent carbon as
impurity along with other impurities like sulphur, phospurous,
silicon and manganese. Pig iron is very hard and brittle
which is unfit for many uses.
Where as
Steel: Steel is an alloy Iron and 0.1 to 1.5% of carbon. Which can
be used for making nails, screws, girders, bridges, railway lines
etc.,
25.
Why is limestone added to the blast furnace?
CaCO3
CaO + CO2
Lime stone on heating produces calcium oxide, CaO which acts as flux
to removes silicon dioxide, SiO2 from ore as slag.
26.
What is 24 carat gold? How will you convert it into 18 carat gold?
24 carat gold means pure gold.
23
18 carat gold can be prepared by mixing 18 parts of god and 6 parts
of copper/silver.
27.
Name an alloy of
a. Aluminum used in the construction of aircrafts
b. Lead used in joining metals for electrical work and
c. Copper used in house hold vessels.
i)
ii)
iii)
28.
Duralumin (Al,Cu,Mg,Mn)
Solder (Pb,Sn)
Brass ( Cu, Zn)
Name the reducing agent which reduces the iron ore in the blast
furnace.
Carbon (or) carbon monoxide
29.
Name the iron compound in hematite.
Write its chemical formula.
Hematite, Fe2O3
30.
A light and strong alloy is required for making the bodies of
aircrafts. Name this alloy. What are its constituents?
Duralumin
Constituents:Aluminum Al,Copper Cu,Magnesium Mg, Manganese Mn
31.
State two ways to prevent rusting of iron.
i) Rusting of Iron can be prevented by painting.
ii) Rusting of Iron can be prevented by applying grease or oil.
iii) Rusting of Iron can be prevented by Cr/Tin/Zinc plating.
iv) Rusting of Iron can be prevented by making it as steel.
32.
Differentiate between metals and non-metals.
Metals
1. Metals are malleable and
ductile
2. Metals are good conductors
of heat and electricity
Non-Metals
1. Non-metals are neither
malleable nor ductile
2. Non-metals are bad conductors
of heat and electricity
Except “c’in the form of
graphite
3. Metals are lustrous
4. Metals forms basic oxide
3. Non-metals are not lustrous
4. Non-metals form acidic
or neutral oxides
5. Metals react with “Hydrogen” 5. Non-metals react with “hydrogen”
to form metal hydrides,
to form non-metal hydrides
which are ionic
which are co-valent
6. Metals form Metals chlorides 6. Non-metals from non-metal
which are ionic
chlorides when are covalent
7. Metals are Electro positive 7. Non-metals are not
Electropositive
33.
What type of oxides is formed when non-metals combine with oxygen?
Non-metals react with oxygen to form acidic oxides or neutral oxide
Eg:
C + O2
CO2(Acidic)
24
34.
35.
C + ½O2
CO(Neutral)
S + O2
SO2(Acidic)
4P + 5O2
2P2O5(Acidic)
Write the chemical reactions that take place during the manufacture
of hydrogen from natural gas.
CH4(g) + H2O(l)
CO(g) + 3H2(g)
CO(g) + H2O(l)
CO2(g) + H2(g)
CO2(g) + H2O(s)
H2CO3(aq)
Give reasons
i) Metals replace hydrogen from dilute acids, whereas non-metals do
not
ii) Carbonate and sulphide ores are usually converted into oxides.
Metals are more electropositive. It means that some metals lose
electrons more readily than hydrogen. So they are able to replace
hydrogen from dilute acids. where as
Zn + 2HCl
ZnCl2+H2
Mg + H2SO4
MgSO4+H2
Non metals are less electropositive (more electronegative) it means
that non-metals gains electrons more readily than hydrogen.
ii)Carbonate and sulphide ores are usually converted into oxides.
It is easier to obtain metal from their oxides than from carbonates or
sulphides by using simple coke (carbon). So carbonates and sulphides are
converted into metal oxides by calcinations and roasting.
36. Name all the products formed when ammonia is passed over heated
Copper (II) oxide.
3CuO
+
2NH3
Copper (II) oxide
Ammonia
3Cu
+
copper
N2
+
nitrogen
3H2O
water
Products: Cu Copper
N2
Nitrogen
H2O Water
37. Ammonia is manufactured from nitrogen and hydrogen by Haber process.
The process is carried out at 200-300 atm and 723-773k
(i)
Give one reason for not using a lower temperature.
(ii) Give one reason for not using a very high pressure.
(iii) How could ammonia be separated from the other two gases?
25
i) At low temperature, the reaction becomes very slow due to which
the
rate of formation of ammonia becomes very slow. A moderate
temperature of around 4500C to 5000C is used in practice for better
yield of NH3
4500c
N2 + 3H2
2NH3
ii) Though the formation of Ammonia is favored by high pressure, it
is very expensive to construct reaction vessel which can withstand
very high pressure, so a moderate pressure of about 200 to 300 Atm
is used in Practice.
300Atm
N2
+
3H2
2NH3
0
45O C
iii) The reaction mixture consisting of N2,H2 & NH3 is cooled to below
00C (below 273k) NH3 gets liquefied and recovered.
38. Describe briefly the Frasch process for the extraction of sulphur.
Fig 14.12 page No: 183
A set of three concentric pipes are bored into sulphur bed.
Superheated is pumped in to bed through outer pipe along with
compressed air through inner pipe. Mixture of molten suphur and
water comes out of the bed through middle pipe. Sulphur is insoluble
in water and can be separated easily.
39. Define allotropy. Name an allotrope of sulphur which is stable at
room temperature.
Existence of of an element in two or more physical forms is called as
allotropy.
i) Rhombic sulphur
ii) Monoclinic sulpher.
Rhombic sulphur is more stable at room temperature.
40. Describe briefly the action of heat one sulphur.
(i) At 388K, it melts to form a clear mobile yellow coloured liquid
which flows like water.
(ii) At about 453K, it becomes thick and orange red and cannot be
poured out even if the vessel is inverted.
(iii) Upto 523K, it remains viscous, but the colour becomes almost
black
(iv) Above 523K the viscousity decreased and at 673 K, it is again a
dark mobile liquid.
(v) Above 713 K, the liquid begins to boil and gives yellow brown
26
Vapours.
41. What would you observe when sulphur dioxide is passed through
(i) lime water;
(ii) acidified potassium dichromate solution?
Write the chemical reactions that take place.
(i) SO2(g) + Ca(OH)2(aq)
CaSO3(s) + H2O(l)
SO2 turns lime water cloudy due to formation of calcium sulphite.
On passing excess SO2 cloudyness disappears due to formation of
calcium hydrogen sulphite which is soluble in water
CaSO3(s) + H2O(l) + SO2(g)
Ca(HSO3)2
ii) 3SO2(g) + 2H+(aq) + Cr2O72-(aq)
3SO42-(aq) + H2O(l) +
2Cr3+(aq)
Orange
green
So2 reduces orange color potassium dichromate solution to green color
chromium sulphate solution
42. In the Contact process for the manufacture of sulphuric. Acid:
(i) Name the catalyst.
(ii) Name the substance in which sulphur trioxide is dissolved.
(iii) Name the substance which is diluted with water.
i) V2O5 Vanadium Pent oxide at 723K
ii) Concentrated H2SO4
(iii) Oleum H2S2O7
43. What happens when a crystal of copper (II) sulphate is placed in conc.
H2SO4? Explain your observation.
CuSO4 5H2O(s)
CuSO4(s)H2O
+
5H2O
(Blue)
(Color less)
Copper (II) sulphate slowly turn white, due to
molecules from copper (II) sulphate crystal.
concentrated H2SO4 acts as good dehydrating agent.
remove of water
It means that
44. Write balanced chemical equation for the three chemical reactions that
take place during the conversion o sulphur dioxide to sulphuric acid
in the Contact process.
V2O5
2 SO2 + O2
2SO3
SO3 + H2SO4
H2S2O7 + H2O
H2S2O7
H2SO4
45. Water should never be added to conc.
H2SO4.
Why?
If water is added to conc. H2SO4 large amount of heat is released at
once, which will convert some water into steam explosively and some
27
is
times it may splash the acid. Hence adding water to conc. H2SO4
dangerous.
Dilution of conc. H2SO4 is done by adding acid to water slowly and
carefully the heat released in this process is slowly absorbed by
large amount of water.
46. Why is sulphuric and known as the “King of Chemicals”?
i)
The use and production of H2SO4 by a country in a financial Year
can be taken as Index for the development of that country in that
year.
ii) There is no Industry which doesn’t use H2SO4 directly or
indirectly
iii) The uses of sulphuric acid are so wide and important.
Hence sulphuric acid is known as “King of Chemicals”
CHAPTER-15
CARBON COMPOUNDS
1.Define the term, functional group and give two examples for it.
Ans:
An atom or a group of atoms on which properties of the carbon
compound depends is known as functional group.
Eg:
- OH
Alcoholic
- CHO
Aldehydic
- CO
Ketonic
- COOH Carboxylic
2. Name the functional groups present in the following compounds.
CH3CH2CH2-OH
CH3CH2CH2COOH
CH3-CH2-CHO
28
CH3COCH2CH2CH3
Ans:
CH3CH2CH2-OH
CH3CH2CH2COOH
CH3-CH2-CHO
CH3COCH2CH2CH3
Alcoholic
Carboxylic
Aldehydic
Ketonic
3. Describe the preparation of ethanol by the fermentation process.
Ans:
Fermentation of sugar is a process in which the sugar molecules are broken
down in the ethylalcohol and carbon dioxide by the action of enzymes
called invertage and zymase which are present in yeast.
Molasses the bi-product of the sugar industry is mixed with suitable
quantity of water and yeast powder. This mixer is kept in a huge steel
tank at 250C to 300C for about 10 to 12 days, during this time fermentation
takes place to form C2H5OH and CO2 gas.
C2H5OH is recovered from this
mixture by distillation.
Invertase
C6H12O6 + C6H12O6
C12 H22 O11 + H2O
(From yeast) Glucose
fructose
Zymase
C6 H22 O16
Glucose & Fructose (from yeast)
2C2H5OH
Ethanol
+
2CO2
4. What are enzymes? Name the enzymes required for fermentation of sugar
cane to ethanol?
Ans:
Enzymes are the chemical substances which acts as biological
catalysts
in bio-chemical reactions.
Eg: 1.Invertage , Zymase, Amylase
and Lactase.
Enzymes required for fermentation of sugar cane to alcohol are
Investase, converts sugar into glucose and fructose.
Invertase
C12 H22 O11
Sugar
C6H12O6 + C6H12O6
(from yeast) Glucose
fructose
Zymase, converts, Glucose and Fructose into C2H5OH and CO2
29
5. Which gas is evolved during the process of fermentation ?
Ans:
CO2; Carbon dioxide.
6. Which of the following reactions represent hydration of ethene?
CH2 + Br2(aq)
BrCH2 – CH2Br
i)
CH2 =
i) O3
ii)
CH2
=
CH2
2HCHO+H2O
Ii H2/pd
H2SO4
iii) CH2
=
CH2 + H2O
Ans CH2
=
CH2 + H2O
CH3 – CH2OH
H2SO4
CH3 – CH2OH
Represents addition of water to ethene(or) hydration of ethene.
07.What is meant by denaturated alcohol ? How is it prepared?
Ans:
Ethyl alcohol (ethanol) made into unfit for drinking is called
denaturated alcohol.
It is prepared by adding poisonous substances like menthol, pyridine,
copper sulphate etc., to ethanol.
08.Give the names of the following :
i) an aldebyde derived from ethane
ii) A ketone derived from butane
iii) The compound obtained by oxidation of ethanol by chromic anhydride
(CrO3); and
iv) The substance formed on catalytic hydrogenation of methanal
Ans:I) Ethanal (Or)Acetaldehyde
ii) 2-Butanone (Or) Butanone-2
iii) Ethanal (Or)Acetaldehyde
iv) Methane
CH3CHO
CH3COCH2CH3
CH3CHO
CH4
09.Describe Tollen’s test. Write the equations of the reactions involved
in this test.
Ans: Tollen’s reagent is ammonical silver nitrate solution containg excess
Ammonium hydroxide.
It is prepared by adding NH4OH to aq AgNO3
solution.
AgNO3
+ 2NH4OH
[Ag(NH3)2]NO3
+
H2O
(Tollen’s reagent)
Tollen’s reagent is mild (weak) oxidizing agent, it oxidizes aldehydes
30
into carboxylic acids.
HCHO + 2[Ag(NH3)2]NO3+ 2NH4OH
HCOOH + 2Ag↓ + 2NH4NO3+4NH3+H2O
Due to the formation of silver (Ag) in the above reaction test tube/
test vessel shines like silver. So this test is also called as silver
mirror test.
11.Give any two uses of methanal ?
Ans:
1. Methanol is used with phenol in the manufacture of bakelite and
other thermosetting plastic.
2. Methanol is used with Ammonia in Preparation of UROTROPINE which is
one of the important medicine for urinary infection.
3. Methanol is used for making formation which is used to preserve
Anatomical specimens.
4. Methanol is used for the manufacture of leather and water proofing
fabrics.
5. Methanol is used in the manufacture of dyes.
10.
Which class of compounds gives positive Fehling’s test? Write the
reactions involved in this test?
Ans:
Aldenydes (-CHO) gives positive Fehlings test.
Aldenydes reacts with Fehlings reagent on heating to form red colored
Cu2O copper(I)oxide and sodium Carboxylate.
HCHO + 2 Cu(OH)2 + NaOH
HCOONa + Cu2O + 3H2O
12. How is propanone prepared commercially? Give the reactions involved in
it?
Ans: Propanone is commercially prepared from cumene by its reaction with
oxygen, followed by treating the product with dil. HCl
CH2
|
CH3 – C – H + O2
|
C6H5
Cumenc
CH3
|
CH3 – C – O – O – H
|
C6H5
CH3
|
CH3 – C – O – O - H
|
C6H5
Cumene hydroperoxide
Dil HCl
C6H5OH + CH3COCH3
31
13. Give an example of an addition reaction of propanone?
i) Addition with Hydrogen Cyanide (HCN)
Ans:Propanone under go addition reaction with HCN to form propanone
Cyanohydrin.
CH3
|
CH3 – C = O + HCN
Propanone
CH3
|
CH3 – C - OH
|
CN
Propanone Cyanohydrin
14. How is ethanoic acid prepared commercially from methanol ?
Ans:
Ethanoic acid is prepared commercially by reaction between methanol and
carbon monoxide in the presence of Iodine - rhodium catalyst.
I2-Rh
CH3OH + CO
CH3COOH
15. Explain the follwing terms:
i)Esterification ii)soponification(iii) decarbodylation (iv)
Polymerisation
Ans:Esterification:- The reaction of carboxylic acid with an alcohol to
form ester in the presence of conc. H2SO4 know as Esterifilation reaction.
CH3COOH + C2H5OH
CH3COOC2H5 + H2O
Saponification : oil or a fat on heating with sodium hydroxide (NaOH)
Solution forms sodium salt of carboxylic acid (soap)and glycerol, this
reaction is know as saponification reaction.
CH2 – O COR
|
CH – O COR + 3NaOH
|
CH2 – O COR
CH2OH
|
CHOH + 3RCOONa
|
CH2OH
Decarboxylation:
Sodium salt of ethanoic acid and soda lime on heating forms methane gas.
This reaction is known as Decarboxylation reaction.
CH3COONa + NaOH
CH4 + Na2CO3
Polymerisation:The processes of formation of a big polymer from monomeric
units is called as polymerization.
32
=
CH2
-CH2-[CH2-CH2]2-CH2n CH2
(Ethene)
(polyethene)
16. Write chemical equations of the reactions of ethanoic acid with
i)sodium (ii) sodium carbonates (iii) ethanol in presence of conc. H2SO4
and (iv) soda lime
Ans: (i) 2 CH3COOH + 2Na
2CH3COONa + H2
(ii) 2CH3COOH + Na2CO3
2CH3COONa + CO2 + H2O
(iii) CH3COOH + C2H5OH
CH3COOC2H5 + H2O
CH4 + Na2CO3
(iv) CH3COOH + NaOH
17. What are polymers? How are they classified ?
Ans:
A polymer is a very big molecule formed by the combination of a large
number of small molecules called monomers.
Eg:- 1. Poly ethene
2. Poly vinyl chloride
3. Rubber
4. Nylon
5. Polyester
Depending upon the type of chemical reaction involved in their preparation
polymers are classified.
Addition Polymers and Condensation polymers.
addition polymers are obtained by the addition of unsaturated compounds
(monomers)
Catalyst
n CH2 = CH2
(CH2 – CH2)n
Δ
n CH2 = CH Cl
n CF2 = CF2
(CH2 – CH)n
|
Cl
(CF2 – CF2)n
n CH2 = CH2
|
CH3
(CH2 – CH2)n
|
CH3
Condensation polymers
Condensation polymers are obtained by the condensation of monomers in
which monomer units are joined together with elimination of H2O,
33
Eg: n HOOC – (CH2)6+ nH2N – (CH2)4COOH – NH2
[HN – (CH2)6-NHCO-(CH2)4-CO-NH]n + nH2O
polyamide (Nylon-66)
Eg:nHO-CH2-CH2-OH+
Ethylene Glycos
nHOOC-C6H4-COOH
Terphthalic acid
(O-CH2-CH2-O-CO-C6H4-Co)n+nH2O
19. Explain the term “vulcanization of rubbers”. What is the advantage of
using vulcanized rubber over natural rubber?
Ans:
01The process of heating natural rubber with sulphur to improve its
property is called vulcanization of rubber.
ADVANTAGES:Natural rubber is very soft and sticky whereas vulcanized rubber is nonsticky and hard.
Natural rubber has low tensile strength whereas vulcanized rubber has high
tensile strength.
Natural rubber has low elasticity whereas vulcanized rubber has high
elasticity.
Natural rubber absorbs more water where as vulcanized rubber absorbs very
less water.
Natural rubber has very low wear and tear resistances. Whereas vulcanized
rubber has high wear and tear resistance.
18. Give two examples of polymers belonging to different classes.
Ans:Addition polymers:
Polyethene
Polyvinylchloride
Teflon
Polypropene
Natural rubber
Neoprene
(CH2-CH2)n
(CH2-CH)n
|
cl
-(CF2 – CF2)n–(CH2-CH)2|
CH3
(CH2-C=CH-CH2)
|
CH3
(CH2-C=CH-CH2)n
Condensation Polymers:
polyamide -(NH-(CH2)6-NHCO-(CH4)4-CO)-n
34
(Nylon 66)
Polyester
-(O-CH2-CH2-OCO-CH4-CO-)n
20. Write the reactions involved in the formation of (i) Polyester and
(ii) pOlyamide
(I) polyester:
nHO – (CH2)2 – CH2 – OH + nHOOC –C6H4 – COOH
Ethylene glycol
Terphthalic acid
(O – CH2 – CH2-OCO – C6H4 –CO )
polyester (Terylene)
n
+nH2O
(ii) Polyamide:
553K
nH=N – (CH2)6 – NH2 + – nHOOC-(CH2)4-COOH
Hexamethylene diamine
Acidic acid
(-HNOC(CH2)4-CONH-(CH2)6)-NHCO-)n
nylon 66
21) Explain the mechanism of the cleansing action of detergents
Answer: Soaps has two parts 1) Long chain alkyl part 2)Ionic part
COO-Na+
Ling chain alkyl
(Hydrophobic)
water repelling
Ionic / Polar
(Hydrophilic)
water attracting
When soaps is applied on only surface long chain alkyl part dissolves
in oil particle to
Micelle .In fact each micelle has negatively charged as shown below
which are easily
Washed away by water.
Ref.Page No 199 Fig No. 15.2 of 10th Std. Science and Technology
35
22. Describe a method for preparation of soap
Ans: Oil/fat is heated with Sodium hydroxide solution. In this process
oil/fat is converted into glycerol and soap. This reaction is known
as
sopanication.
Heat
Oil/fat
+Sodium hydroxide
Soap +
Glycerol
CH2-OCOR
|
CH-OCOR
|
CH2-OCOR
+
3NaOH
CH2OH
|
CHOH
|
CH2OH
+ 3RCOONa
When the soponification process is complete, somesodium chloride solution
is added to solution to separate soap.
Raw materials: i) Animal fat or vegetable oil
ii) Sodium hydroxide
iii) Sodium chloride