Question 1

The First Law of Thermodynamics states that:

Accepted Answer

A)   Molecules move faster as temperature increases.
B)   The total entropy of the universe is increasing.
C)   Energy transfers from hotter objects to cooler objects.
D)   Samples with different temperatures that come in contact with one another will reach thermal equilibrium.
E)   The total energy of the universe is constant.F) D) and E)
G) A) and B)

Question 2

Based on the following thermochemical equation, which statement is false?

Accepted Answer

A)   The thermochemical equation represents a physical change.
B)   The enthalpy change for the gas condensing into a liquid is known.
C)   The internal energy of the surroundings increases.
D)   The pressure for the process is known.
E)   The enthalpy change is endothermic.F) A) and E)
G) A) and D)

Question 3

Determine the heat of reaction for the process

using the information given below:

Accepted Answer

A)   -1074.0 kJ
B)   -22.0 kJ
C)   22.2 kJ
D)   249.8 kJ
E)   1074.0 kJF) C) and D)
G) B) and C)

Question 4

What is the enthalpy change when 175 g of C3H8 are burned in excess O2? 3H8 are burned in excess O2?   A)  -1.71 × 107 kJ B)  -1.79 × 10-3 kJ C)  -3.47 × 100 kJ D)  -3.89 × 105 kJ E)  -8.82 × 103 kJ" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -1.71 × 107 kJ
B)   -1.79 × 10-3 kJ
C)   -3.47 × 100 kJ
D)   -3.89 × 105 kJ
E)   -8.82 × 103 kJF) All of the above
G) B) and E)

Question 5

Which of the following is not an example of kinetic energy?

Accepted Answer

A)   the motion of a molecule
B)   a golf ball sitting on a tee
C)   the vibration of an object
D)   a brick falling from the top of a building
E)   the motion of electrons through a wireF) All of the above
G) B) and E)

Question 6

Based on the following thermochemical equation below, which statement is false? 3. C)  The value of 92.22 kJ applies to the reaction of two moles of N2 and three moles of H2. D)  Per mole of N2, DH° = -46.11 kJ. E)  Per mole of H2, DH° = -15.37 kJ." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   For the reverse process, DH° = + 46.11 kJ.
B)   The value of 46.11 kJ applies to the formation of two moles of NH3.
C)   The value of 92.22 kJ applies to the reaction of two moles of N2 and three moles of H2.
D)   Per mole of N2, DH° = -46.11 kJ.
E)   Per mole of H2, DH° = -15.37 kJ.F) A) and B)
G) A) and C)

Question 7

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g-1 °C-1) .

Accepted Answer

A)   0.485 g
B)   0.607 g
C)   485 g
D)   607 g
E)   2.43 × 103 gF) None of the above
G) A) and E)

Question 8

A 0.100 mole sample of CH4 reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g-1 °C-1. 4 reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g-1 °C-1.   A)  4.35 × 10-3°C B)  7.56°C C)  10.2°C D)  31.6°C E)  43.5°C" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   4.35 × 10-3°C
B)   7.56°C
C)   10.2°C
D)   31.6°C
E)   43.5°CF) A) and B)
G) A) and C) E

Question 9

The complete combustion of 1.47 g of methanol produces 29.3 kJ of heat. Determine the DH° for the reaction and its sign.

Accepted Answer

A)   -938 kJ
B)   -638 kJ
C)   -1.35 kJ
D)   +638 kJ
E)   +938 kJF) A) and B)
G) B) and D)

Question 10

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g-1 at 0 °C; the specific heat of water = 4.184 J g-1 °C-1; the heat of vaporization of water = 2260 J g-1 at 100 °C.

Accepted Answer

A)   30100 J
B)   22600 J
C)   4180 J
D)   3330 J
E)   343 JF) A) and B)
G) A) and C)

Question 11

Which of the following is an example of potential energy?

Accepted Answer

A)   atoms vibrating back and forth around a specific location
B)   a rock rolling down a mountain
C)   a fat molecule stored in the body
D)   electrons flowing through an electrical conductor
E)   the sound of a dog barkingF) A) and C)
G) A) and D) C

Question 12

A 20.0 g sample of aluminum (specific heat = 0.902 J g-1 °C-1)  with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Accepted Answer

A)   74.8°C
B)   72.3°C
C)   26.2°C
D)   24.9°C
E)   23.7°CF) B) and E)
G) B) and D)

Question 13

In a(n) _____________ reaction, the energy of bond breaking is greater than the energy of bond making.

Accepted Answer

The answer of In a(n) _____________ reaction, the energy of...

Question 14

Which substance has the highest molar heat capacity?

Accepted Answer

A)   copper (specific heat = 0.385 J g-1 °C-1) 
B)   iron (specific heat = 0.451 J g-1 °C-1) 
C)   silver (specific heat = 0.232 J g-1 °C-1) 
D)   lead (specific heat = 0.128 J g-1 °C-1) 
E)   aluminum (specific heat = 0.902 J g-1 °C-1) F) All of the above
G) A) and B)

Question 15

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g-1 °C-1) .

Accepted Answer

A)   490 J
B)   979 J
C)   1.47 × 103 J
D)   7.65 × 103 J
E)   5.98 × 104 JF) A) and D)
G) A) and B)

Question 16

Determine the heat of reaction for the process

using the information given below:

Accepted Answer

A)   -295.3 kJ
B)   -29.2 kJ
C)   +29.2 kJ
D)   +295.3 kJ
E)   +398.4 kJF) B) and E)
G) B) and D)

Question 17

Which statement about energy is false?

Accepted Answer

A)   Thermodynamics is the science of working and heating processes.
B)   Working and heating are processes that transfer energy.
C)   Chemical reactions are processes that transfer energy
D)   The chemical energy of foods and fuels is a type of potential energy.
E)   The thermal energy of nanoscale objects is a type of potential energy.F) C) and E)
G) All of the above

Question 18

The quantity of energy required to increase the temperature of one gram of a sample by 1°C is called the _____________.

Accepted Answer

specific heat

Question 19

In an endothermic reaction, heat is transferred from the _____________ to the _____________.

Accepted Answer

surroundin...

Question 20

The temperature of a 21.6 g sample of a metal rises 6.04°C when 58.8 J of energy is applied to it. What is the identity of the metal?

Accepted Answer

A)   silver (specific heat = 0.232 J g-1 °C-1) 
B)   copper (specific heat = 0.385 J g-1 °C-1) 
C)   iron (specific heat = 0.451 J g-1 °C-1) 
D)   lead (specific heat = 0.128 J g-1 °C-1) 
E)   aluminum (specific heat = 0.902 J g-1 °C-1) F) C) and D)
G) B) and E)

Exam 6: Energy and Chemical Reactions

The First Law of Thermodynamics states that:

Correct AnswerverifiedShow Answer

Based on the following thermochemical equation, which statement is false?

Correct AnswerverifiedShow Answer

Determine the heat of reaction for the process using the information given below:

Correct AnswerverifiedShow Answer

What is the enthalpy change when 175 g of C3H8 are burned in excess O2?

Correct AnswerverifiedShow Answer

Which of the following is not an example of kinetic energy?

Correct AnswerverifiedShow Answer

Based on the following thermochemical equation below, which statement is false?

Correct AnswerverifiedShow Answer

Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g-1 °C-1) .

Correct AnswerverifiedShow Answer

A 0.100 mole sample of CH4 reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g-1 °C-1.

Correct AnswerverifiedE

The complete combustion of 1.47 g of methanol produces 29.3 kJ of heat. Determine the DH° for the reaction and its sign.

Correct AnswerverifiedShow Answer

How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g-1 at 0 °C; the specific heat of water = 4.184 J g-1 °C-1; the heat of vaporization of water = 2260 J g-1 at 100 °C.

Correct AnswerverifiedShow Answer

Which of the following is an example of potential energy?

Correct AnswerverifiedC

A 20.0 g sample of aluminum (specific heat = 0.902 J g-1 °C-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Correct AnswerverifiedShow Answer

In a(n) _____________ reaction, the energy of bond breaking is greater than the energy of bond making.

Correct AnswerverifiedShow Answer

Which substance has the highest molar heat capacity?

Correct AnswerverifiedShow Answer

Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g-1 °C-1) .

Correct AnswerverifiedShow Answer

Determine the heat of reaction for the process using the information given below:

Correct AnswerverifiedShow Answer

Which statement about energy is false?

Correct AnswerverifiedShow Answer

The quantity of energy required to increase the temperature of one gram of a sample by 1°C is called the _____________.

Correct Answerverifiedspecific heat

In an endothermic reaction, heat is transferred from the _____________ to the _____________.

Correct Answerverifiedsurroundin...View AnswerShow Answer

The temperature of a 21.6 g sample of a metal rises 6.04°C when 58.8 J of energy is applied to it. What is the identity of the metal?

Correct AnswerverifiedShow Answer

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What is the enthalpy change when 175 g of C₃H₈ are burned in excess O₂?

Correct Answer
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Determine the quantity of ice required to absorb exactly 50 kJ of energy when the ice warms from -50.0°C to -10.0°C (specific heat of ice = 2.06 J g^-1 °C^-1) .

Correct Answer
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A 0.100 mole sample of CH₄ reacts completely in a calorimeter having a heat capacity of 783 J/°C. The calorimeter contains 254 g of water. Determine the temperature increase of the calorimeter. The specific heat of water = 4.184 J g^-1 °C^-1.

Correct Answer
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E

Correct Answer
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How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g^-1 at 0 °C; the specific heat of water = 4.184 J g^-1 °C^-1; the heat of vaporization of water = 2260 J g^-1 at 100 °C.

Correct Answer
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C

A 20.0 g sample of aluminum (specific heat = 0.902 J g^-1 °C^-1) with an initial temperature of 48.6°C is heated with 427 J of energy. What is the final temperature of the sample?

Correct Answer
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Correct Answer
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Determine the amount of heat required to raise the temperature of a 153 g bar of gold by 50.0°C (specific heat of gold = 0.128 J g^-1 °C^-1) .

Correct Answer
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Correct Answer
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specific heat

In an endothermic reaction, heat is transferred from the _ to the _.

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surroundin...
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