Download BP_3rd quarter final review

3rd quarter final
Review
UNIT 6
The Mole
1. Avogadro's number of representative
particles is equal to one ____.
a.
b.
c.
d.
e.
Gram
Mole
Kilogram
Atom
two of the above are true
2. All of the following are equal to
Avogadro's number EXCEPT ____.
a.
b.
c.
d.
the number of atoms of bromine in 1 mol Br2
the number of atoms of gold in 1 mol Au
the number of molecules of nitrogen in 1 mol N2
the number of molecules of carbon monoxide in 1
mol CO
e. the number of formula units of magnesium
chloride in 1 mol MgCl2
3. How many moles of gold atoms are in
2.0 x 1023 atoms of gold?
a.
b.
c.
d.
e.
6.022 x 1023
1.0
0.50
0.33
2 (6.022 x 1023)
4. How many formula units are in 0.50 mol
of sodium chloride?
a.
b.
c.
d.
e.
6.022 x 1023
3.0 x 1023
1.20 x 1024
3.0
0.50 / 6.022x 1023
5. The mass of a mole of NaCl is the ____
a.
b.
c.
d.
atomic mass
molecular mass
molar mass
average mass
6. What is the molar mass of carbon
dioxide?
a.
b.
c.
d.
28.01 g/mol
40.02 g/mol
44.01 g/mol
76.01 g/mol
7. What is the molar mass of calcium
hydroxide?
a.
b.
c.
d.
41 g/mol
57 g/mol
58 g/mol
74 g/mol
8. What is the number of moles of argon
atoms in 120 g of argon?
a.
b.
c.
d.
e.
0.50 mol
2.0 mol
3.0 mol
120 x (6.022 x 1023) mol
6.022 x 1023 mol
9. Pencil lead is composed of graphite,
which is made of carbon. How many
atoms of carbon can be found in 6.0 g of
pencil lead?
a. 1.0
b. 3.01 x 1023
c. 6.022 x 1023
d. 6 x 12 (6.022 x 1023)
10. The lowest whole-number ratio of the
elements in a compound is called the
____.
a.
b.
c.
d.
empirical formula
molecular formula
mole ratio
lowest common denominator formula
11. Which of the following is NOT an
empirical formula?
a.
b.
c.
d.
e.
C2N2H7
C3H9O6
Na2SO4
Sb2S3
at least two of the above
12. Which of the following is NOT true
about empirical and molecular formulas?
a. The molecular formula of a compound can be
the same as its empirical formula.
b. The molecular formula of a compound can be
some whole-number multiple of its empirical
formula.
c. Several compounds can have the same
empirical formula, but have different molecular
formulas.
d. The empirical formula of a compound can be
triple its molecular formula.
e. at least two of the above are not true
13. If the molar mass of a compound is
266.7 g/mol and its empirical formula is
B2H5, determine the molecular formula.
a.
b.
c.
d.
e.
23
10
B4H10
B6H15
B20H50
a. Atoms  only contains element
b. Molecules  any covalent compound or nonmetal only
c. formula units  any ionic compound or metal and
nonmetal combined
d. Ions  any ions with + or - charge
1. 1 mole CuCO3 = 5 atoms
1. Incorrect
2. If there is 1 formula unit, then it contains 5 atoms
2. 1 mole O2 = 32.00 g O2
1. Correct
2. 1 mole of substance has molar mass
3. 1 mole CH3OH = 6.022 x 1023 atoms
1. Incorrect
2. If there are 6.022 x 1023 molecules, then it is correct
a. Difference?
a. empirical formula is the simplest ratio of the
element in a compound.
b. You can’t simplify.
c. Molecular formula is the simple whole number
multiple of its empirical formula.
d. You can simplify.
i. If the substance is MF, write its empirical
formula.
ii. H2O
iii. K2SO4
iv. C3H6
v. C6H12O3
a. a color change
b. release of a gas
c. release of energy in form of heat or
light
d. all of the above
a.
b.
c.
d.
(s) = solid, (aq) = gas
(g) = gas, (l) = liquid
(aq) = aqueous, (l) = lethal
all of these
a. This is a single replacement
reaction.
b. The cations of both reactants will
switch places.
c. A white solid will form from two
solutions.
d. Two of the above are true
17. (NH4)2Cr2O7  N2 + H2O + Cr2O3
a.2, 4, 1, 2
b.1, 1, 4, 1
c.1, 1, 4, 2
d.2, 2, 4,1
18. C8H18 + O2  CO2 + H2O
a.2, 4, 16, 18
b.1, 1, 4,1
c.1, 1, 4, 2
d.2, 25, 16, 18
19. Cu + AgNO3  Ag + Cu(NO3)2
a.2, 4, 1, 2
b.1, 1, 4, 1
c.1, 2, 2, 1
d.2, 2, 4, 1
20. Use the activity series, which of
the following is correct?
a.
b.
c.
d.
Br2 < I2
Na < Mg
H2 < Na
Li < Cu
a.
b.
c.
d.
Cu + NaCl 
Ca + HCl 
I2 + KBr 
they all take place
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
PbI2
Fe(OH)3
AgCl
(NH4)2SO4
PbNO3
AgNO3
Cu(C2H3O2)2
Ca3(PO4)2
NaCl
CuCO3
A+BCAC+B
2. Single Replacement
3. A+BAB
4. Synthesis
5. ABA+B
6. Decomposition
7. AB+CDAD+CB
8. Double Replacement
9. AB+O2AO2+B2O
10. Combustion
1.
__ a) __ CaCl2 + __ Na3PO4  __ NaCl + __ Ca3(PO4)2
DR a) 3 CaCl2 + 2 Na3PO4  6 NaCl + 1 Ca3(PO4)2
___ b) __ NaHCO3  __ Na2CO3 + __ H2O + __ CO2
D b) 2 NaHCO3  1 Na2CO3 + 1 H2O + 1 CO2
___ c) ___ C6H14 + ___ O2  ___ CO2 + ___ H2O
C c) 2 C6H14 + 19 O2  12 CO2
+ 14 H2O
_____ d) _____ Na
+ _____ Cl2 
_____ NaCl
S d) 2 Na + 1 Cl2  2 NaCl
___ e) ___ Fe + ___ AgNO3  __ Ag + ___ Fe(NO3)3
SR e) 1 Fe + 3 AgNO3  3 Ag + 1 Fe(NO3)3
____ f) ___ H2 (g)
+ __ O2 (g)
 ___ H2O (l)
__S_ f) _2__ H2 (g) + _1_ O2 (g)  _2__ H2O (l)
___ g) ____ NH3 (g) 
___ H2 (g)
+ ____ N2 (g)
D g) 2 NH3 (g)  3 H2 (g) + 1 N2 (g)
__ h) __ H2SO4 (aq) +__ Ba(OH)2 (aq)
 __ BaSO4 (s) + __H2O (l)
_DR_ h) _1_ H2SO4 (aq) +_1_ Ba(OH)2 (aq)
 _1_ BaSO4 (s) + _2_H2O (l)
__ i) __ K (s) + __ H2O (l)
 __ KOH (aq) + __ H2 (g)
_SR_ i) _2_ K (s) + _2_ H2O (l)
 _2_ KOH (aq) + _1_ H2 (g)
__ j) __ CaCO3 (s)  __ CaO (s) + __ CO2 (g)
_D_ j) _1_ CaCO3 (s)  _1_ CaO (s) + _1_ CO2 (g)
__ k) __ C12H22O11 (s) +__ O2 (g)
 __ CO2 (g) + __ H2O (l)
_C_ k) _1_ C12H22O11 (s) +_12_ O2 (g)
 _12_ CO2 (g) + _11_ H2O (l)
CHEMISTRY
Review for midterm
UNIT 8
Stoichiometry
25. In the reaction: 2 Al(OH)3 + 3
Ca(NO3)2  3 Ca(OH)2 + 2 Al(NO3)3. If 6
moles of aluminum nitrate were
produced, how many moles of calcium
nitrate were consumed?
A. 3 moles
B. 6 moles
C. 9 moles
D. 12 moles
E. 15 moles
26. If 10 moles of methane combusts
in an excess of oxygen, how many
moles of water would be produced?
A. 2. 5 moles
B. 5 moles
C. 10 moles
D. 20 moles
E. 40 moles
27. In the unbalanced equation:
__CuSO4 + __K3PO4
 __K2SO4 + __Cu3(PO4)2
if 12 moles of copper (II) sulfate
reacted with an excess of potassium
phosphate, how many moles of
potassium sulfate are produced?
27. In the unbalanced equation:
3CuSO4 + 2K3PO4
 3K2SO4 + 1Cu3(PO4)2
if 12 moles of copper (II) sulfate reacted
with an excess of potassium phosphate,
how many moles of potassium sulfate are
produced?
A.
B.
C.
D.
E.
4 moles
8 moles
12 moles
16 moles
24 moles
28. If 4 moles of potassium carbonate
reacts with an excess of iron (III)
hydroxide, how many moles of
potassium hydroxide will be
produced?
A. 1 mole
B. 2 moles
C. 4 moles
D. 8 moles
E. 12 moles
29. Consider the unbalanced equation:
_Cu + _AgNO3  _Cu(NO3)2 + _Ag .
If 3 moles of silver are produced,
how many moles of copper were
used?
29. Consider the unbalanced equation:
1Cu + 2AgNO3  1Cu(NO3)2 + 2Ag .
If 3 moles of silver are produced,
how many moles of copper were
used?
A. 1 mole
B. 1.5 moles
C. 2 moles
D. 2.5 moles
E. 3 moles
30. In a chemical reaction, the amount
of product that is calculated and could
be formed is called the
A. limiting reactant
B. excess reactant
C. actual yield
D.theoretical yield
31. In the following:
CH4 + 2O2  CO2 + 2H2O, how many grams
of CO2 are formed when 10.0 moles of
oxygen reacts with excess methane?
A. 220 g
B. 110g
C. 44 g
D.22 g
32. When making cheeseburgers, how
many complete cheeseburgers can be
made using 101 buns, 50 patties, 75
slices of cheese, and 43 tomato slices?
(recipe: 2 buns, 1 patty, 1 slice of
cheese, 1 tomato slice)
A.
B.
C.
D.
51
50
38
43
33. When making cheeseburgers,
which is limiting if there are 101 buns,
40 patties, 70 slices of cheese, and 43
tomato slices? (recipe: 2 buns, 1
patty, 1 slice of cheese, 1 tomato slice)
A. Buns
B. Patties
C. Cheese
D. tomato
34. Use the answer from #33. When
making cheeseburgers, what is the
theoretical yield if there are 101 buns,
40 patties, 70 slices of cheese, and 43
tomato slices? (recipe: 2 buns, 1
patty, 1 slice of cheese, 1 tomato slice)
A.
B.
C.
D.
101
40
70
43
35. Use the answer from #33, 34. If you
made 30 cheeseburgers, what is the
percent yield if there are 101 buns, 40
patties, 70 slices of cheese, and 43
tomato slices? (recipe: 2 buns, 1 patty, 1
slice of cheese, 1 tomato slice)
A.
B.
C.
D.
25%
50%
75%
100%
36. In the equation
NaCl (aq) + AgNO3 (aq)  NaNO3(aq) +
AgCl (s)
how many moles of NaCl would be required
to form 3.3 moles of AgCl?
A. 1.0
B. 3.3
C. 6.6
D. 1.7
37. In an experiment, 100 g of bromine
react with excess lithium in the reaction:
2Li + Br2  2LiBr. You calculated that you
would produce 150 g of sodium chloride,
but you only collected 105 g of sodium
chloride from the experiment. Which set up
represents the calculation for the percent
yield of lithium bromide?
A.
C.
B.
D.
For questions 38-43, use the following
information:
a student immersed a piece of zinc wire in
a solution of silver hydroxide, producing
silver crystals and a solution of zinc (II)
hydroxide.
1 Zn (s) + 2 AgOH (aq) 2 Ag (s) +1 Zn(OH)2 (aq)
(balanced)
a student immersed a piece of zinc wire in
a solution of silver hydroxide, producing
silver crystals and a solution of zinc (II)
hydroxide.
1 Zn (s) + 2 AgOH (aq) 2 Ag (s) +1 Zn(OH)2 (aq)
39. If I want to produce 24.6 moles of silver, how
many moles of silver hydroxide should I use?
Mole to mole
24.6 mol
Ag
2 mol AgOH
X
2 mol Ag
=
24.6 mol
AgOH
a student immersed a piece of zinc wire in
a solution of silver hydroxide, producing
silver crystals and a solution of zinc (II)
hydroxide.
Mass to mass
1 Zn (s) + 2 AgOH (aq) 2 Ag (s) +1 Zn(OH)2 (aq)
40. If I produced 87.7 grams of zinc (II) hydroxide,
how many grams of zinc did I react?
87.7 g
Zn(OH)2
X
1 mol
Zn(OH)2
99.41g X
Zn(OH)2
1 mol
Zn
1 mol
Zn(OH)2
65.38 g
Zn
x
1 mol
Zn
=
57.7 g Zn
1 Zn (s) + 2 AgOH (aq)
2 Ag (s) +1 Zn(OH)2 (aq)
2 numbers
2 equations
41. If I reacted 25.6 grams of silver hydroxide with
25.6 grams of zinc, what was my limiting reactant?
1 mol
AgOH
25.6 g
X
X
AgOH
124.88 g
AgOH
1 mol
Zn
2 mol Ag
25.6
X
X
g Zn
65.38
g Zn
2 mol
AgOH
2 mol
Ag
1 mol
Zn
=
=
0.205 mol
Ag
25.6 g
AgOH is
limiting
0.783 mol
Ag
1 Zn (s) + 2 AgOH (aq)
2 Ag (s) +1 Zn(OH)2 (aq)
Theoretical yield
Gram to gram
42. If I have 40.5 grams of zinc and an excess of
silver hydroxide, what is my theoretical yield of
silver?
40.5 g
Zn
1 mol
Zn
X
65.38g X
Zn
2 mol
Ag
1 mol
Zn
107.87
g Ag
x
1 mol
Ag
=
133 g Ag
1 Zn (s) + 2 AgOH (aq)
Find theoretical
yield
2 Ag (s) +1 Zn(OH)2 (aq) Find percent yield
43. If I have 40.5 grams of zinc and excess silver
hydroxide but only produced 5.0 grams of silver
crystals, what was my percent yield?
1 mol Zn
40.5 g
Zn
X
107.87
g Ag
2 mol Ag
x
65.38g X
Zn
1 mol Zn
1 mol
Ag
P = Actual / Theoretical x 100
5.0 g
133 g
X
100
=
3.8 %
=
133 g Ag
44. In the unbalanced equation,
__ C12H22O11 +__ O2  __ CO2 + __ H2O,
How many grams of water would be
formed when 1.0 mole of sucrose reacts
with excess oxygen?
Mole to mass
44. In the unbalanced equation,
1 C12H22O11 + 12 O2  12 CO2 + 11 H2O,
How many grams of water would be
formed when 1.0 mole of sucrose reacts
with excess oxygen?
1.0 mol
X
C12H22O11
11 mol
H 2O
1 mol
C12H22O11
X
18.02 g
H 2O
1 mol H2O
=
198.22 g
H2O