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Chemistry Final Review

Total questions: 59

Worksheet time: 1hrs 11mins

Name
Class
Date
1.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

2.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

3.

When solid NaCl is stirred into water, which of the following is NOT true?

a)

Individual sodium and chloride ions are present.

b)

The solution will conduct electricity.

c)

The solution will taste salty.

d)

The NaCl will fail to dissociate (separate into ions)

4.

In writing the chemical equation for a reaction that produces a precipitate, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

5.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

6.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

Which compound would not form ions in the complete ionic equation?

a)

PbI2

b)

KNO3

c)

Pb(NO3)2

d)

KI

7.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

b)

Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

c)

Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

d)

Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

8.

When some ionic compounds form through reactions in solution, they fall out as a ___

a)

consolidated element

b)

heavy sludge

c)

dense discharge

d)

solid precipitate

9.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
10.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
11.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
12.
Which of these results in the formation of a precipitate?
a)
AgNO3(aq)  +  NaOH(aq)→
b)
BaNO3(aq)  +  CaCl2(aq)→
c)
NaNO3(aq)  +  KOH(aq)→
d)
More than one of these form precipitates
13.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
14.
What is the result of the reaction between potassium bromide and ammonium sulfide?
a)
potassium sulfide precipitates
b)
ammonium bromide precipitates
c)
potassium ammonium precipitates
d)
no precipitate is formed
15.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)?

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

16.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
17.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
18.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
19.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
20.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

21.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
22.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
23.

What is the Molar Mass of Potassium Sulfide?..... :-) You get to figure out the formula.

a)

110.262 g/mol

b)

71.164 g/mol

c)

174.258 g/mol

d)

158.259 g/mol

24.

Which of the following is needed to determine the molar mass of a molecule?

a)

Types of elements in the molecule

b)

Quantity of elements in the molecule

c)

Mass of the elements in the molecule

d)

All are correct and needed.

25.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
26.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

27.

Calculate the molar mass of Cu2O.

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

28.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
29.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
30.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
31.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
32.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
d)
Yield
33.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
d)
Yield
34.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
35.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
36.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
37.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
38.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
39.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
40.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
41.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
42.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

43.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
44.
2 NaCl + Pb(NO3)2 --> 2 NaNO3 + PbCl2
 
How many grams of lead II chloride are produced from the reaction of 15.3 g of NaCl and 60.8 g of Pb(NO3)2? 
a)
21.5g
b)
51.1g
c)
43.4g
d)
36.4g
45.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
46.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
47.

Identify the limiting and excess reactants in the reaction shown.

a)

N2 is limiting and H2 is excess. 

b)

H2 is limiting and N2 is excess. 

c)

NH3 is both limiting and excess.

d)

There is no limiting reactant. 

48.
A reactant that remains after a chemical reaction stops
a)
stoichiometry
b)
mole ratio
c)
excess reactant
d)
limiting reactant
49.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

50.

How many Joules of energy are required to change 10 gram of liquid water from 20 C to 90 C?

a)

1400 J

b)

2800 J

c)

210,000 J

d)

1,400,000 J

51.
The specific heat of aluminum is 0.21 J/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
52.

If the specific heat of water is 4,184 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

112,575.9 K

53.
The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?
a)
12.82 °C
b)
24.12°C
c)
351 °C
54.
The specific heat of aluminum is 0.21 cal/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
55.
Enthalpy is energy absorbed or relased during a chemical reaction as
a)
light.
b)
heat.
c)
sound.
d)
pressure.
56.

Using the equations below:

C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ

what is ∆H (in kJ) for the following reaction?

MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

57.

Using the equations below

Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ

2Cu(s) + O2(g) → Cu2O(s) ∆H = –170 kJ

what is the value of ∆H (in kJ) for the following reaction?

2CuO(s) → Cu2O(s) + 1/2O2(g)

a)

142

b)

15

c)

-15

d)

-142

58.

Consider the following equations.

Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ

What is the ∆H value (in kJ) for the following reaction?

MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

59.

The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide.

C(s) +O2(g) → CO2(g) ΔH = –x kJ mol–1

CO(g) + O2(g) → CO2(g) ΔH = –y kJ mol–1

What is the enthalpy change, in kJ mol–1, for the oxidation of carbon to carbon monoxide?

C(s) + O2(g) → CO(g)

a)

x + y

b)

-x - y

c)

y - x

d)

x - y

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