Download Chemistry 11 Review

Chemistry 11
Course Review
Chemistry 11 – Course Review
Names and Formulas for Compounds
1.
2.
Write the correct formula for the following compounds:
a)
ammonium chloride.................................................... ________________________
b)
copper (II) sulphate .................................................... ________________________
c)
zinc bromide .............................................................. ________________________
e)
Lithium oxide.............................................................. ________________________
f)
iron (III) carbonate...................................................... ________________________
h)
calcium hydroxide ...................................................... ________________________
Write the correct names for the following compounds:
a)
Mn(SO4)2..................................... _________________________________________
b)
PbCrO4 ....................................... _________________________________________
c)
H2CO3 ......................................... _________________________________________
d)
C4H10...........................................
e)
NaHCO3 ...................................... _________________________________________
f)
AlF3 ............................................. _________________________________________
g)
(NH4)3PO4 ................................... _________________________________________
h)
Ba(OH)2....................................... _________________________________________
______________________________________
The Mole Concept
1.
Make the following conversions, clearly showing your steps. Include proper units in all of
your work and in your answer.
a)
133.44 grams of PCl5 = ? moles
Answer ___________________________
b)
2.56 grams of O2 = ? Litres at SLC
Answer ___________________________
Chemistry 11—Course Review
Page 1
Chemistry 11
c)
Course Review
320 mL of 1.5 M HCl solution = ? mole
Answer ___________________________
d)
0.5696 g of Na2O(s) dissolved in 40.0 mL water = ? Molar concentration
Answer __________________________
Chemical Reactions
1.
Balance and classify the following equations as synthesis (S), decomposition (D), single
displacement (SD), double replacement (DD), neutralization (N) or combustion (C).
NH3
+

O2
NO
+
H2O

(NH4)2C2O4
+
AlCl3
C14H30
+
O2

CO2
Fe
+
HNO3

Fe(NO3)3
P4
+
Cl2

Na2Cr2O7 +
H3PO4
Ba(ClO4)2
C7H15OH

NaCl

Ca(OH)2

+
+
+
NH4Cl
H2O
+
H2
PCl3
HCl
+
Al2(C2O4)3
Ba
O2
+

+
CrCl3
Ca3(PO4)2
Cl2
CO2
+
+
+
+
H2O
+
Cl2
H2O
O2
H2O
2. Write a balanced chemical equation for each of the following (first classify each reaction to
assist in predicting the product). Indicate the state of each substance by checking its
solubility where needed.
a)
potassium sulphate is mixed with zinc (III) nitrate
b)
liquid propanol (C3H7OH) is burned in air
c)
copper oxide is heated and is decomposed into it’s elements
d)
a piece of zinc is placed in a test-tube containing a solution of silver nitrate
Chemistry 11—Course Review
Page 2
Chemistry 11
3.
Course Review
e)
sulfuric acid is mixed with calcium carbonate
f)
silver sulfate is reacted with ammonium chloride
g)
aluminium reacts with chlorine gas
h)
hydrochloric acid reacts with strontium hydroxide
State whether each of the following are exothermic or endothermic.
HCl + 432 kJ  H + Cl
Answer ___________________________
C12H22O11 + 12 O2  12CO2 + 11H2O
Energy (kJ)
H2O(s)  H2O(l)
H = -5638 kJ Answer ___________________
Answer ___________________________
A + B
AB
Reaction Proceeding 
Answer ___________________________
H= 65.7 kJ
CD  C + D
Answer ___________________________
Stoichiometry
1.
Given the following balanced equation, answer the questions following it:
2NF3(g)
a)
+
3H2(g)
 N2(g)
+ 6HF(g)
If 5.5 moles of H2 are reacted, how many moles of NF3 will be consumed?
Answer ____________
b)
In order to produce 0.47 moles of HF, how many moles of NF3 would be consumed?
Answer ____________
Chemistry 11—Course Review
Page 3
Chemistry 11
c)
Course Review
If you needed to produce 180.6 g of N2, how many moles of H2 would you need to
start with?
Answer ____________
2.
Given the following balanced equation, answer the questions following it:
HBrO3
a)
+
5 HBr
 3 H2O(l)
+ 3 Br2(g)
If 3.56 moles of HBr are reacted, how many Litres of Br2 will be formed at STP?
Answer ______________________
b)
In order to produce 3.311 x 1024 molecules of Br2, what mass of HBr is needed?
Answer ______________________
3.
Given the following balanced chemical equation, answer the question below it.
MgCO3 (s) +
a)
2HCl (aq)
 CO2 (g) + H2O (l) +
MgCl2(aq)
What mass of MgCO3 will react completely with 15.0 mL of 1.5 M HCl?
Answer _______________________
4.
Given the following balanced equation, answer the questions below it.
3 Cu(s) + 8HNO3(l)  3 Cu(NO3)2(aq) + 2NO(g) + 4 H2O(l)
a)
If 317.5 grams of Cu are reacted, find out how many grams of HNO3, are required.
Answer _______________________
Chemistry 11—Course Review
Page 4
Chemistry 11
Course Review
Bonding and Solubility
1.
2.
3.
In an ionic bond, electrons are
a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole
Answer ________
In a covalent bond, electrons are
a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole
Answer ________
In a polar covalent bond, electrons are
a. shared equally by two atoms
b. shared unequally by two atoms
c. transferred from a metal to a non-metal
d. transferred from a non-metal to a metal
e. closer to one end of a molecule, forming a temporary dipole
Answer ________
4.
What physical evidence do we have that ionic bonds are very strong?
5.
Write electron-dot diagrams for:
PBr3(covalent)
SF2(covalent)
CH3CH3(covalent)
6. Describe the difference between a saturated and unsaturated solution.
7. Explain how heat, in general, affects solubility.
8. Explain the chemical differences that would make KI more soluble than NaCl.
9. Describe why HBr would be more soluble than CH4 in water at the same temperature.
Chemistry 11—Course Review
Page 5
Chemistry 11
Course Review
Reaction Kinetics
1.
For each of the following reactions find at least two quantities or properties which could
be monitored in order to measure the rate of reaction
a) 3H2(g) + N2(g)  2NH3(g)
b) CaCO3(s) 
CaO(s) +
___________________________________________
CO2(g) _______________________________________
c) 2NO2(g)  N2O4(g) _________________________________________________
2.
A chemist wishes to determine the rate of reaction of sodium hydrogen carbonate with
hydrochloric acid. Write the balanced reaction:
NaHCO3(s) + HCl(aq)

A piece of NaHCO3 is dropped into 1.00 L of HCl(aq) and the following data were obtained:
Time
Mass of NaHCO3
0s
0.020 g
4s
0.018 g
8s
0.016 g
12 s
0.014 g
16 s
0.012 g
20 s
0.010 g
a)
Calculate the Rate of Reaction in grams of NaHCO3 consumed per second.
Answer___________________
b) Calculate the Rate of Reaction in moles of NaHCO3 consumed per second.
Answer___________________
c)
What will happen to the [HCl] as the reaction proceeds? _________________________
3. When pentane (C5H12) is burned in air (oxygen), the products carbon dioxide and water
are formed.
a) Write a balanced formula equation for this reaction.
_____________________________________________________________________
Chemistry 11—Course Review
Page 6
Chemistry 11
Course Review
b) If pentane is consumed at an average rate of 2.16 grams/s, determine the rate of
consumption of pentane in moles/s.
Answer___________________
c) If pentane is consumed at an average rate of 0.030 moles/s, determine the rate of
consumption of oxygen in moles/s.
Answer___________________
d) If pentane is consumed at an average rate of 0.030 moles/s, determine the rate of
production of CO2 in grams/s.
Answer__________________
4. a) In a room filled with H2 and O2 there are about 1032 collisions per second. Explain why
the reaction between H2 and O2 at room temperature is so slow as to be unnoticeable!
b) Suggest two ways in which this reaction could be speeded up.
5. Use the following Potential Energy Diagram to answer all the questions below:
a) What is the value of ∆H for the reaction ?
Answer_______________
b) What is the value of the activation energy for the reaction?
Answer_______________
Chemistry 11—Course Review
Page 7
Chemistry 11
Course Review
c)
Which species is the activated complex?
Answer________________
d)
Which set of species has the lowest potential energy?
Answer________________
e)
Is the reaction as written endothermic or exothermic?
Answer _______________
f)
What is the minimum energy needed to start the reaction
Answer________________
g)
What happens to the kinetic energy (speed) of A2 and B as the reaction proceeds past the
activated complex and toward the products?
h)
Answer________________
For A2 and B to form the activated complex they must have the proper energy and
the proper _______________________________________________________
i)
j)
Draw another curve on the graph with another colour showing the catalyzed
What effect did the catalyst have on the activation energy for the forward reaction?
____________________________________________________________
k) What effect did the catalyst have on the ∆H of the forward reaction? ___________________
6.Describe what happens to the kinetic energy, potential energy and the total energy of reactant
molecules as they approach each other.
7. A small piece of zinc react with 2.0 M HCl to produce 12.0 mL of H2 gas in 30.0 seconds.
Calculate the rate of reaction
a) In mL of H2/second
Answer__________________________
b) In moles of H2/second
Answer__________________________
8. Which of the following reactions is most likely to have the greatest rate at room temperature?
a) Ag+(aq) + I- (aq)  AgI(s)
b) H2 (g) + Cl2 (g)  2HCl (g)
c) C3H8 (g) + 5O2 (g) 
3CO2 (g) + 4H2O (g)
d) Fe (s) + S(s) 
FeS (s)
Answer________________. Explain how you arrived at your answer._______________
______________________________________________________________________
Chemistry 11—Course Review
Page 8
Chemistry 11
9.
Course Review
Describe what happens to two reactant particles which collide with less energy than the
Activation Energy.
__________________________________________________________________
Acids and Bases
1.
Write balanced formula equations for the reactions which happen when the following are
mixed:
a) sodium hydroxide and phosphoric acid
_____________________________________________________________________
b) sulphuric acid and aluminum hydroxide
_____________________________________________________________________
c) Fe(OH)3 + HNO3
_____________________________________________________________________
2.
Write the formula for a proton _________________________
3.
Write the formula for a hydrated proton __________________
4.
Write the formula for a hydronium ion ___________________
5.
Give the definition of an acid______________________________________________
6.
Give the definition of a base ______________________________________________
7.
Given the equation: HCO3- + H2S  H2CO3 + HSa)
The acid on the left side is ______________
b)
The base on the left side is ______________
8.
What would have the higher [H3O+] in water, 10.0 M HClO4 or 1.0 M HClO4 __________
9.
What would have the higher [H3O+] in water, 10.0 M NaOH or 10.0 M HNO2? _________
10.
What would have the higher [H3O+] in water, 1.0 M HBr or 1.0 M H2SO4? ___________
11.
What is the [H3O+] and the pH of a 0.001 M of nitric acid solution.
Answer _____________________________
Chemistry 11—Course Review
Page 9
Chemistry 11
Course Review
12.
13.45 mL of 0.200 M NaOH is required to neutralise 25.0 mL of a solution which is
known to have HCl. Calculate the original [HCl]. Show all your steps.
13.
13.45 mL of 0.200 M HCl is required to neutralise 25.0 mL of a solution which is
known to have Ba(OH)2. Calculate the original [Ba(OH)2]. Show all your steps.
14.
13.45 mL of 0.200 M Sr(OH)2 is required to neutralise 25.0 mL of a solution which is
known to have HNO3. Calculate the original [HNO3]. Show all your steps.
15.
What volume of 0.100 M NaOH would be required to neutralise 35.0 mL of a
0.231M solution of H2C2O4. Show all your steps.
16.
Calculate the mass of NaOH which is required to neutralise 15.00 mL of
0.350 M H2SO4?
Chemistry 11—Course Review
Page 10
Chemistry 11
17.
Course Review
Consider the following 0.100 M solutions:
I. HF
II. HBr
III. H2SO4
The equivalence point is reached when 10.00 mL of 0.100 M NaOH has been
added to 10.00 mL of solutions
A. II only
B. I and II only
C. II and III only
D. I, II and III
18.
Given the following data table:
Beaker
1
2
3
a)
Volume
10.0 mL
20.0 mL
50.0 mL
Contents
0.1 M Ba(OH)2
0.05 M KOH
0.2 M NaOH
Which beaker would require the greatest volume of 0.1M HCl for complete
neutralization? ________________ (1 mark)
b)
Which beaker would require the least volume of 0.1M HCl for complete
neutralization? _______________ (1 mark)
19. What volume of a 2.8 M sulfuric acid solution is needed to prepare 250 mL of 0.6 M sulfuric
acid?
Gas Laws
1. A sample of gas collected in a 180 mL container has a pressure of 78.9 kPa. What would the
volume of this gas be at 106.5 kPa?
2. A 325 mL volume of gas is collected at 46oC. What volume would this sample occupy at
85oC?
Chemistry 11—Course Review
Page 11