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Chem Final Review- No Lechat or Acids/Bases

Total questions: 157

Worksheet time: 8hrs 12mins

Name
Class
Date
1.
In the equation,          2Mg + O2 ---> 2MgO, which are the reactants?
a)
Mg and O
b)
MgO
c)
Mg and MgO
d)
O and MgO
2.
Balance this equation,            Al2O3 ---> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 ---> 2Al + 3O2 
c)
2Al2O3 ---> 4Al + 3O2 
d)
3Al2O3 ---> 2Al + O2 
3.
Name this reaction, CO2 + H2O --> H2CO3 
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Combustion
4.
Name this reaction, Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single Replacement
c)
Double Replacement
d)
Decomposition
5.
Balance this equation:  H2 + N2 → NH3
a)
 H2 + 4N2 → NH3
b)
 H2 + 3N2 → 2NH3
c)
 3H2 + N2 → 2NH3
d)
 2H2 + 2N2 → 2NH3
6.
Which is a Decomposition Reaction?
a)
AB --> A + B
b)
ab ----> a + B
c)
AB + CD ----> AC +BC
d)
AB+ C ----> AC + B
7.
Balance this equation:  H2 + N2 → NH3
a)
 H2 + 4N2 → NH3
b)
 H2 + 3N2 → 2NH3
c)
 3H2 + N2 → 2NH3
d)
 2H2 + 2N2 → 2NH3
8.
NaI +BaCl2 -----> NaCl +BaI2 is an example of?
a)
Combustion
b)
Single replacement
c)
Double replacement
d)
Decomposition
9.
Balance this reaction: ____ HCN + ____ CuSO4 ---->____ H2SO4 + ____ Cu(CN)2
a)
2,1,1,2
b)
2,1,1,1
c)
1,2,2,1
d)
1,2,1,1
10.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
11.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
12.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
13.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
14.
What is the percentage of oxygen in carbon dioxide? (CO2)
a)
27.3%
b)
72.7%
c)
30%
d)
70%
15.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
16.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
17.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
18.
What is the percentage of chlorine in sodium chloride? (NaCl)
a)
60.7%
b)
39.3%
c)
60%
d)
40%
19.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
20.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
21.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
22.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
23.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
24.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
25.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
26.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
27.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
28.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
29.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
30.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
31.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
32.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
33.
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
34.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
35.
Which conversion factor should be used to solve the following, "How many moles of argon atoms are present in 11.2 L of argon gas at STP?"
a)
1 mol = 22.4 L 
b)
1 mol = 39.95 g
c)
1 mol = 6.02x1023 atoms
d)
More than 1
36.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
37.
Which conversion factor should be used to solve the following, "Find the mass in grams of 2.00 x 1023 molecules of F2."
a)
1 mol = 22.4 L 
b)
1 mol = 38.00 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
38.
What operation will be performed when converting from moles to another unit?
a)
addition
b)
subtraction
c)
multiplication
d)
division
39.
Which expression below show the correct method of determining the percent composition of Sodium in Na2CO3?
a)
%Na = (22.99g/106g) x 100
b)
%Na = (22.99g/106) / 100
c)
%Na = (45.98g/106g) x 100
d)
%Na = (106/45.98g) x 100
40.
What operation will be performed when converting from a unit to moles.
a)
addition 
b)
subtraction
c)
multiplication
d)
division
41.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
42.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
43.
The number 6.02 x 1023, which is the number of particles found in a mole. 
a)
molar mass
b)
mole
c)
Avogadro's number
d)
hydrate
44.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
45.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
46.
How many grams are in 3.3 mol of Potassium Sulfide?
a)
360 g
b)
454 g
c)
238 g
d)
132 g
47.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
48.
Which of the following would have the highest number of moles?
a)
4g CO2
b)
15g H2O
c)
22g NaCl
d)
100g AgCl
49.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

50.
Find the percent composition of hydrogen in (NH4)2S.
a)
11.8%
b)
41.1%
c)
47.1%
51.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
52.
A container with a volume of 893 L contains how many moles of air at STP?
a)
20003.2 L
b)
39.9 L
c)
22.4 L
d)
none of the choices
53.
Which of the following dimensional analysis setups will correctly convert 2.50 moles of sodium to grams of sodium?
a)
A
b)
B
c)
C
d)
D
54.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
55.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
56.
Which represents the greatest mass of sulfur?
a)
1 gram of sulfur
b)
1 molecule of sulfur
c)
0.5 mole of sulfur
d)
6.02 x 1023 atoms of sulfur
57.
How many grams of Hydrogen are there in 25 moles of water?
a)
25 g
b)
450 g
c)
18 g
d)
50 g
58.
Which of the following dimensional analysis setups will correctly convert 4.00x1023atoms of cobalt to moles of cobalt? How many moles of colbalt are there?
a)
setup B : 0.6644mol Co
b)
setup A: 2.41x1047mol Co
c)
setup A : 0.664mol Co
d)
setup B: 2.41x1047mol Co
59.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
60.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
61.
100 degrees Celsius is equal to _______ Kelvin. 
a)
0 K
b)
273 K
c)
173 K
d)
373 K
62.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
63.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
64.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
65.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
66.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
67.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
68.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
69.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
70.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
71.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
72.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
73.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K
74.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
75.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
76.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
77.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
78.
Which of the following factors increases only the effectiveness of collisions?
a)
temperature
b)
catalysts
c)
concentration
d)
particle size
79.
Reaction rate means...
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
80.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
81.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
82.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
83.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
84.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is conctant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
85.

Identify the incorrect statement about achieving equilibrium.

a)

achieved when product and reactant concentrations are equal

b)

achieved when forward and reverse reaction rates are same

c)

achieved when concentration of reactants is stable/constant

d)

achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

86.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
87.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
88.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
89.
It is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
a)
reversible reaction
b)
irreversible reaction
c)
decomposition reaction
d)
synthesis
90.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
91.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
92.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
93.
Which of the two graphs reaches equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
94.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
95.
During equilibrium, the rates of the forward and the reverse reaction are ________
a)
the same 
b)
unequal
c)
unequal for exothermic reactions
d)
unequal for endothermic reactions
96.
If a reaction is reversible and has reached equilibrium, what can be said about the amounts of reactants and products?
a)
some reactant, some product
b)
no reactant, all product
c)
all reactant, no product
97.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
98.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
99.
What is the activation energy?
a)
the quantity of heat absorbed in a reaction
b)
the minimum energy needed to begin a reaction
c)
the energy given off after reactants collide.
d)
both the energy and frequeny of collisions in increased
the energy difference between reactants and products
100.

What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?

a)

0.21 M

b)

30 M

c)

4.8 M

d)

20.8 M

101.
What is the molality of a solution containing 1.3 mol in 13.4 kg of solution?
a)
9.7 m
b)
17.42 m
c)
0.097 m
102.
What is the molarity of 122.5 g of AlCl3 in 1.0 L of solution?
a)
1.225 M
b)
0.92 M
c)
0.1225 M
103.

What is the molality of 1.2 g of HCl in 750 g of solution?

a)

0.04 m

b)

0.00004 m

c)

0.0016 m

104.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
105.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
106.

What mass of solute is needed to make 75.0 g of a 3.4% solution?

a)

2.55 g

b)

22 g

c)

0.05 g

107.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
108.

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

109.
Moles per kilograms is the unit used for measuring
a)
enthalpy
b)
effervescence
c)
molarity
d)
molality
110.
The unit of measurement for molality is
a)
molars
b)
molals
c)
moles
d)
mollas
111.

A solution that is considered dilute would be....

a)

Dark in color

b)

Have a strong scent

c)

Have a large amount of solute

d)

Have a small amount of solute

112.

The substance being dissolved in a solution.

a)

sands

b)

solute

c)

solvent

d)

alloy

113.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
114.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
115.
air is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
116.

A solute is........

a)

any substance that will dissolve in a solvent

b)

anysubstance that will not dissolve in a solvent

c)

the same as a solvent

d)

is always a solid

117.

Water is known as

a)

the universal solute

b)

something you drink to stay young

c)

the universal solvent

d)

something you drink to get old

118.
A solution that can hold more solute  is called
a)
saturated
b)
supersaturated
c)
unsaturated
d)
insoluble
119.
Something that cannot be dissolved into a solution is called
a)
soluble
b)
insoluble
c)
solution
d)
suspension
120.

When a solution cannot dissolve more solute, it is called

a)

saturated

b)

supersaturated

c)

unsaturated

d)

solvent

121.

Which of the following would increase the amount of solute dissolved?

a)

decreasing temperature

b)

increasing temperature

c)

decreasing amount of solvent

d)

increasing amount of solute

122.

What could you do to increase the solubility of a gas?

a)

increase pressure

b)

decrease pressure

c)

increase temperature

d)

do nothing

123.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

124.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

125.

molality is defined as ________________________

a)

the moles of solute per kilogram of solvent

b)

moles of solute per liter of solution

c)

mass of solute/ mass of solution

d)

mass of solute/ mass of solvent X 100

126.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
127.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

128.

The _____ is the thing being dissolved.

a)

solute

b)

solvent

129.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
130.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

131.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

132.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

133.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

134.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

135.

How do you convert from grams to moles?

a)

Divide by the molar mass

b)

Multiply by the molar mass

c)

Divide by Avogadro's number

d)

Multiply by Avogadro's number

136.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

137.

What are the units of molality?

a)

M

b)

m

c)

Ml

d)

Mr

138.

Heat of Reaction

a)

The heat released after burning 1 mole of a substance.

b)

The amount of heat needed to melt 1 mole of a solid.

c)

The heat released by 1 mole of a substance as it changes from a liquid to a solid.

d)

The heat released or absorbed during a chemical reaction.

139.

Enthalpy (H)

a)

The heat content of a system at constant pressure.

b)

A chemical equation that includes the amount of heat released or absorbed during the reaction.

c)

The heat released or absorbed during a chemical reaction.

d)

The heat released after burning 1 mole of a substance.

140.

Endothermic reactions feel

a)

warm

b)

cold

141.

Exothermic reactions feel

a)

warm

b)

cold

142.

Chemical reactions that release energy. The ΔH reaction is negative.

a)

Specific Heat

b)

Endothermic Reaction

c)

Exothermic Reaction

d)

Enthalpy

143.

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

144.

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

145.

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

146.

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

147.

Which of the following statements are true for the reaction:

SO2(g) + 1/2O2(g) ↔ SO3(g)

ΔH = –92 kJ mol-1

Where ↔ indicates that the reaction can proceed in the forward and the reverse direction.

a)

The forward and reverse reaction both produce 92 kJ of energy.

b)

Oxidizing 2 moles of SO2 would produce twice as much energy.

c)

The reverse reaction has an enthalpy of +92 kJ mol-1.

d)

Collecting the SO3 produced in the liquid state would not change the measured enthalpy.

148.

The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1

What is the enthalpy change, in kJ mol–1, for the reaction below?

P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

149.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
c)
Sometimes
150.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
c)
nothing happens
d)
it gets colder
151.

A chemical reaction that requires energy is a(n)

a)
exothermic reaction 
b)
endothermic reaction 
c)
over reaction 
d)
redox reaction
152.

The enthalpies of combustion of C(s), H2(g) and C4H9OH(l) (in kJmol-1) are as follows   C(s) + O2(g)   --->  CO2(g)   ∆H=a H2(g) + ½O2(g)   --->   H2O(l)  ∆H=b C4H9OH(l) + 6O2(g)   --->   4CO2(g) + 5H2O(l)  ∆H=c

What is the enthalpy change for the reaction shown below?   4C(g) + 5H2(l) + ½O2(g)   --->   C4H9OH(l)

a)
c – 4a – 5b
b)
2a + 10b - c
c)
4a + 5b - c
d)
2a + 5b + c
153.

If N2 (g) + 2O2 (g) ⟶\longrightarrow   2NO2(g) has a ΔHrxn \Delta H_{rxn\ }  = 68, then what is the ΔHrxn\Delta H_{rxn}  if you reverse the reaction?

a)

86 kJ

b)

- 86 kJ

c)

68 kJ

d)

-68 kJ

154.
a)
-804.6
b)
-202.3
c)
-296.1
d)
-233.0
155.
a)
-233
b)
-11.3
c)
-805
d)
-226
156.
a)
226
b)
255
c)
233
d)
11.3
157.
a)
-296.1
b)
226
c)
-11
d)
255.95

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