Question 1

For a particular process that is carried out at constant pressure,q = 140 kJ and w = -30 kJ.Therefore,

Accepted Answer

A)  ΔE = 110 kJ and ΔH = 140 kJ. 
B)  ΔE = 140 kJ and ΔH = 110 kJ. 
C)  ΔE = 140 kJ and ΔH = 170 kJ. 
D)  ΔE = 170 kJ and ΔH = 140 kJ. 
A)  ΔE = 110 kJ and ΔH = 140 kJ. 
B)  ΔE = 140 kJ and ΔH = 110 kJ. 
C)  ΔE = 140 kJ and ΔH = 170 kJ. 
D)  ΔE = 170 kJ and ΔH = 140 kJ.

Question 2

Hydroelectric power plants produce nearly ________ percent of U.S.electricity.

Accepted Answer

A)  2 
B)  10 
C)  7 
D)  19 
E)  11 
A)  2 
B)  10 
C)  7 
D)  19 
E)  11

Question 3

Which of the following statements is TRUE?

Accepted Answer

A)  State functions do not depend on the path taken to arrive at a particular state. 
B)  DErxn can be determined using constant volume calorimetry. 
C)  Energy is neither created nor destroyed, excluding nuclear reactions. 
D)  ΔHrxn can be determined using constant pressure calorimetry. 
E)  All of the above are true. 
A)  State functions do not depend on the path taken to arrive at a particular state. 
B)  DErxn can be determined using constant volume calorimetry. 
C)  Energy is neither created nor destroyed, excluding nuclear reactions. 
D)  ΔHrxn can be determined using constant pressure calorimetry. 
E)  All of the above are true.

Question 4

Which of the following processes is exothermic?

Accepted Answer

A)  the ionization of a melting snow atom 
B)  the breaking of a boiling of water bond 
C)  the boiling of water 
D)  the condensation of water 
E)  All of the above processes are exothermic. 
A)  the ionization of a melting snow atom 
B)  the breaking of a boiling of water bond 
C)  the boiling of water 
D)  the condensation of water 
E)  All of the above processes are exothermic.

Question 5

Match between columns
                        Premises: -w
+ΔE
+w
-ΔE
+ q
-q

Accepted Answer

The Answer of work done on the system by the is...

Question 6

Identify what a bomb calorimeter measures.

Accepted Answer

A)  measures ΔH for combustion solutions 
B)  measures ΔE for combustion reactions 
C)  measures ΔH for oxidation solutions 
D)  measures ΔT for oxidation solutions 
E)  measures ΔE for reduction reactions 
A)  measures ΔH for combustion solutions 
B)  measures ΔE for combustion reactions 
C)  measures ΔH for oxidation solutions 
D)  measures ΔT for oxidation solutions 
E)  measures ΔE for reduction reactions

Question 7

A 21.8 g sample of ethanol (C2H5OH)is burned in a bomb calorimeter,according to the following reaction.If the temperature rises from 25.0 to 62.3°C,determine the heat capacity of the calorimeter.The molar mass of ethanol is 46.07 g/mol. C2H5OH(l)+ 3 O2(g)→ 2 CO2(g)+ 3 H2O(g)ΔH°rxn = -1235 kJ

Accepted Answer

A)  4.99 kJ/°C 
B)  5.65 kJ/°C 
C)  63.7 kJ/°C 
D)  33.1 kJ/°C 
E)  15.7 kJ/°C 
A)  4.99 kJ/°C 
B)  5.65 kJ/°C 
C)  63.7 kJ/°C 
D)  33.1 kJ/°C 
E)  15.7 kJ/°C

Question 8

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 25.0°C to 70.0°C.What is the specific heat of benzene?

Accepted Answer

A)  1.14 J/(g ∙ °
C)  
B)  1.72 J/(g ∙ °
C)  
C)  3.50 J/(g ∙ °
C)  
D)  5.33 J/(g ∙ °
C)  
A)  1.14 J/(g ∙ °
C)  
B)  1.72 J/(g ∙ °
C)  
C)  3.50 J/(g ∙ °
C)  
D)  5.33 J/(g ∙ °
C)

Question 9

Give the units of molar heat capacity.

Accepted Answer

A)  J/°F 
B)  J/g °C 
C)  J/mole°C 
D)  g/°C 
E)  gmole °F 
A)  J/°F 
B)  J/g °C 
C)  J/mole°C 
D)  g/°C 
E)  gmole °F

Question 10

Using the following equation for the combustion of octane,calculate the heat associated with the combustion of 100.0 g of octane assuming complete combustion.The molar mass of octane is 114.33 g/mole.The molar mass of oxygen is 31.9988 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

Accepted Answer

A)  -535.4 kJ 
B)  -4819 kJ 
C)  -602.3 kJ 
D)  -385.5 kJ 
E)  -11018 kJ 
A)  -535.4 kJ 
B)  -4819 kJ 
C)  -602.3 kJ 
D)  -385.5 kJ 
E)  -11018 kJ

Question 11

How much energy is required to decompose 800 g of PCl3,according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g)→ P4(s)+ 6 Cl2(g)ΔH°rxn = +1207 kJ

Accepted Answer

A)  2.71 × 103 kJ 
B)  4.53 × 103 kJ 
C)  6.72 × 103 kJ 
D)  1.76 × 103 kJ 
E)  5.90 × 103 kJ 
A)  2.71 × 103 kJ 
B)  4.53 × 103 kJ 
C)  6.72 × 103 kJ 
D)  1.76 × 103 kJ 
E)  5.90 × 103 kJ

Question 12

Where does the energy absorbed during an endothermic reaction go?

Accepted Answer

During an endothermic reaction,the produ

Question 13

How much heat is absorbed when 40.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO2(g)→ CS2(l)+ 4 CO(g)ΔH° = 239.9 kJ

Accepted Answer

A)  159.8 kJ 
B)  239.9 kJ 
C)  798.7 kJ 
D)  1918 kJ 
A)  159.8 kJ 
B)  239.9 kJ 
C)  798.7 kJ 
D)  1918 kJ

Question 14

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g): ΔH°f (kJ/mol) 2 SO2(g)+ O2(g)→ 2 SO3(g)ΔH°rxn = -198 kJ
SO2(g)-297

Accepted Answer

A)  -792 kJ/mol 
B)  -248 kJ/mol 
C)  -495 kJ/mol 
D)  -578 kJ/mol 
E)  -396 kJ/mol 
A)  -792 kJ/mol 
B)  -248 kJ/mol 
C)  -495 kJ/mol 
D)  -578 kJ/mol 
E)  -396 kJ/mol

Question 15

Determine the specific heat capacity of an alloy that requires 69.3 kJ to raise the temperature of 150.0 g alloy from 450 K to 550 K.

Accepted Answer

A)  3.20 J/g°C 
B)  2.00 J/g°C 
C)  4.62 J/g°C 
D)  1.79 J/g°C 
E)  7.20 J/g°C 
A)  3.20 J/g°C 
B)  2.00 J/g°C 
C)  4.62 J/g°C 
D)  1.79 J/g°C 
E)  7.20 J/g°C

Question 16

How much energy is evolved during the formation of 816 g of Al2O3,according to the reaction below? Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

Accepted Answer

A)  6.82 × 103 kJ 
B)  9.90 × 103 kJ 
C)  5.60 × 103 kJ 
D)  4.50 × 102 kJ 
E)  6.60 × 102 kJ 
A)  6.82 × 103 kJ 
B)  9.90 × 103 kJ 
C)  5.60 × 103 kJ 
D)  4.50 × 102 kJ 
E)  6.60 × 102 kJ

Question 17

A 6.50-g sample of liquid water at 25.0 C is heated by the addition of 145 J of energy.The final temperature of the water is ________°C.The specific heat capacity of liquid water is

Accepted Answer

A)  118 
B)  25.2 
C)  -19.7 
D)  30.3 
E)  5.34 
A)  118 
B)  25.2 
C)  -19.7 
D)  30.3 
E)  5.34

Question 18

Which of the following signs on q and w represent a system that is doing work on the surroundings,as well as gaining heat from the surroundings?

Accepted Answer

A)  q = +, w = - 
B)  q = -, w = + 
C)  q = +, w = + 
D)  q = -, w = - 
E)  None of these represent the system referenced above. 
A)  q = +, w = - 
B)  q = -, w = + 
C)  q = +, w = + 
D)  q = -, w = - 
E)  None of these represent the system referenced above.

Question 19

The specific heat capacity of solid copper metal is 0.385 J/gK.How many joules of heat are needed to raise the temperature of a 1.15-kg block of copper from 25.0°C to 66.0°C?

Accepted Answer

A)  1.22 × 105 J 
B)  18.2 J 
C)  1.82 × 104 J 
D)  8.17 × 10-6 J 
E)  0.00817 J 
A)  1.22 × 105 J 
B)  18.2 J 
C)  1.82 × 104 J 
D)  8.17 × 10-6 J 
E)  0.00817 J

Question 20

Determine the final temperature of a gold nugget (mass = 376 g)that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost.The specific heat capacity of gold is 0.128 J/g°C.

Accepted Answer

A)  133 K 
B)  398 K 
C)  187 K 
D)  297 K 
E)  377 K 
A)  133 K 
B)  398 K 
C)  187 K 
D)  297 K 
E)  377 K

Exam 6: Thermochemistry

For a particular process that is carried out at constant pressure,q = 140 kJ and w = -30 kJ.Therefore,

Hydroelectric power plants produce nearly ________ percent of U.S.electricity.

Which of the following statements is TRUE?

Which of the following processes is exothermic?

Identify what a bomb calorimeter measures.

A 21.8 g sample of ethanol (C2H5OH)is burned in a bomb calorimeter,according to the following reaction.If the temperature rises from 25.0 to 62.3°C,determine the heat capacity of the calorimeter.The molar mass of ethanol is 46.07 g/mol. C2H5OH(l)+ 3 O2(g)→ 2 CO2(g)+ 3 H2O(g)ΔH°rxn = -1235 kJ

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 25.0°C to 70.0°C.What is the specific heat of benzene?

Give the units of molar heat capacity.

How much energy is required to decompose 800 g of PCl3,according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful. 4 PCl3(g)→ P4(s)+ 6 Cl2(g)ΔH°rxn = +1207 kJ

Where does the energy absorbed during an endothermic reaction go?

How much heat is absorbed when 40.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO2(g)→ CS2(l)+ 4 CO(g)ΔH° = 239.9 kJ

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g): ΔH°f (kJ/mol) 2 SO2(g)+ O2(g)→ 2 SO3(g)ΔH°rxn = -198 kJ SO2(g)-297

Determine the specific heat capacity of an alloy that requires 69.3 kJ to raise the temperature of 150.0 g alloy from 450 K to 550 K.

How much energy is evolved during the formation of 816 g of Al2O3,according to the reaction below? Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

A 6.50-g sample of liquid water at 25.0 C is heated by the addition of 145 J of energy.The final temperature of the water is ________°C.The specific heat capacity of liquid water is

Which of the following signs on q and w represent a system that is doing work on the surroundings,as well as gaining heat from the surroundings?

The specific heat capacity of solid copper metal is 0.385 J/gK.How many joules of heat are needed to raise the temperature of a 1.15-kg block of copper from 25.0°C to 66.0°C?

Determine the final temperature of a gold nugget (mass = 376 g)that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost.The specific heat capacity of gold is 0.128 J/g°C.

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Chemical Quantities and Aqueous Reactions

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The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

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How much energy is required to decompose 800 g of PCl₃,according to the reaction below? The molar mass of PCl₃ is 137.32 g/mol and may be useful. 4 PCl₃(g)→ P₄(s)+ 6 Cl₂(g)ΔH°_rxn = +1207 kJ

How much heat is absorbed when 40.00 g of C(s)reacts in the presence of excess SO₂(g)to produce CS₂(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO₂(g)→ CS₂(l)+ 4 CO(g)ΔH° = 239.9 kJ

Use the ΔH°_f and ΔH°_rxninformation provided to calculate ΔH°_f for SO₃(g): ΔH°_{f (kJ/mol)} 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)ΔH°_rxn= -198 kJ SO₂(g)-297

How much energy is evolved during the formation of 816 g of Al₂O₃,according to the reaction below? Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ