Question 1

A mass of 1.250 g of benzoic acid (C7H6O2) was completely combusted in a bomb calorimeter. If the heat capacity of the calorimeter was 10.134 kJ/K and the heat of combustion of benzoic acid is -3226 kJ/mol, calculate (to three decimal places) the temperature increase that should have occurred in the apparatus.

Accepted Answer

Temperatur...

Question 2

.

Accepted Answer

A)   iron
B)   copper
C)   granite
D)   gold
E)   waterF) C) and E)
G) All of the above

Question 3

Your favorite candy bar, Gummy Beakers, contains 1.2 *106 J of energy while your favorite soft drink, Bolt, contains 6.7 *105 J. If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt, what percent of your 2000 Calorie daily food intake is left for broccoli, beans, beef, etc.?

Accepted Answer

A)   53%
B)   47%
C)   27%
D)   11%
E)   0%F) A) and B)
G) A) and C)

Question 4

A system initially has an internal energy E of 501 J. It undergoes a process during which it releases 111 J of heat energy to the surroundings, and does work of 222 J. What is the final energy of the system, in J?

Accepted Answer

A)   168 J
B)   390 J
C)   612 J
D)   834 J
E)   cannot be calculated without more informationF) C) and D)
G) A) and B)

Question 5

The combustion of glucose (C6H12O6)  with oxygen gas produces carbon dioxide and water. This process releases 2803 kJ per mole of glucose. When 3.00 mol of oxygen react in this way with glucose, what is the energy release in kcal? (Hint: Write a balanced equation for the combustion process.)

Accepted Answer

A)   223.5 kcal
B)   335.3 kcal
C)   1402 kcal
D)   2012 kcal
E)   5858 kcalF) B) and E)
G) A) and E) B

Question 6

The standard state of a substance in aqueous solution is a 1 M solution.

Accepted Answer

A) True 
 B)False

Question 7

$\Delta$H does not depend on the path of a reaction, but $\Delta$E does.

Accepted Answer

A) True 
 B)False  False

Question 8

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25 °\degree° C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g ? K)

Accepted Answer

A)   3 °\degree° C
B)   14 °\degree° C
C)   22 °\degree° C
D)   47 °\degree° C
E)   None of these choices is correct. F) A) and E)
G) B) and D)

Question 9

A system delivers 225 J of heat to the surroundings while delivering 645 J of work. Calculate the change in the internal energy,  Δ\DeltaΔ E, of the system.

Accepted Answer

A)   -420 J
B)   420 J
C)   -870 J
D)   870 J
E)   -225 J F) All of the above
G) A) and B)

Question 10

A piece of copper metal is initially at 100.0 °\degree° C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 °\degree° C. After stirring, the final temperature of both copper and water is 25.0 °\degree° C. Assuming no heat losses, and that the specific heat (capacity)  of water is 4.18 J/(g ? K) , what is the heat capacity of the copper in J/K?

Accepted Answer

A)   2.79 J/K
B)   3.33 J/K
C)   13.9 J/K
D)   209 J/K
E)   None of these choices is correct. F) A) and C)
G) C) and D)

Question 11

For all processes, both q and $\Delta$E will have the same sign.

Accepted Answer

A) True 
 B)False

Question 12

For a reaction in a sealed, rigid container, $\Delta$H is always greater than $\Delta$E.

Accepted Answer

A) True 
 B)False

Question 13

Consider the equation $\Delta$E = q + w. Explain fully the meaning of all three terms in the equation, and also the implied sign convention for q and w.

Accepted Answer

E is the internal energy of a system, i....

Question 14

A system that does no work but which receives heat from the surroundings has:

Accepted Answer

A)   q Δ\DeltaΔ E > 0
B)   q > 0,  Δ\DeltaΔ E 
C)   q =  Δ\DeltaΔ E
D)   q = - Δ\DeltaΔ E
E)   w =  Δ\DeltaΔ E F) All of the above
G) B) and D)

Question 15

A system contracts from an initial volume of 15.0 L to a final volume of 10.0 L under a constant external pressure of 0.800 atm. The value of w, in J, is:

Accepted Answer

A)   -4.0 J
B)   4.0 J
C)   -405 J
D)   405 J
E)   4.05 *103 JF) B) and E)
G) D) and E)

Question 16

For which one of the following reactions will  Δ\DeltaΔ H be approximately (or exactly)  equal to  Δ\DeltaΔ E?

Accepted Answer

A)   H2(g)  + Br2(g)   →\rightarrow→ 2HBr(g) 
B)   H2O(l)   →\rightarrow→ H2O(g) 
C)   CaCO3(s)   →\rightarrow→ CaO(s)  + CO2(g) 
D)   2H(g)  + O(g)   →\rightarrow→ H2O(l) 
E)   CH4(g)  + 2O2(g)   →\rightarrow→  CO2(g)  + 2H2O(l)  F) B) and D)
G) A) and B)

Question 17

Which of the following is not a state function?

Accepted Answer

A)   internal energy
B)   volume
C)   work
D)   pressure
E)   enthalpyF) None of the above
G) A) and D)

Question 18

Standard heats (enthalpies) of formation of compounds, $\Delta$H$\degree$f, may be positive or negative.

Accepted Answer

A) True 
 B)False

Question 19

In which of the following processes is  Δ\DeltaΔ H =  Δ\DeltaΔ E ?

Accepted Answer

A)   Two moles of ammonia gas are cooled from 325 °\degree° C to 300 °\degree° C at 1.2 atm.
B)   One gram of water is vaporized at 100 °\degree° C and 1 atm.
C)   Two moles of hydrogen iodide gas react to form hydrogen gas and iodine gas in a 40-L container.
D)   Calcium carbonate is heated to form calcium oxide and carbon dioxide in a container with variable volume.
E)   One mole of solid carbon dioxide sublimes to the gas phase. F) A) and B)
G) C) and D) C

Question 20

Clearly state the thermodynamic standard state of
A) an element or compound.
B) a solute.

Accepted Answer

a. Standard state is the stabl...

Exam 6: Thermochemistry: Energy Flow and Chemical Change

Correct Answer
verified
Temperatur...
View Answer

.

Correct Answer
verified

Your favorite candy bar, Gummy Beakers, contains 1.2 10⁶ J of energy while your favorite soft drink, Bolt, contains 6.7 10⁵ J. If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt, what percent of your 2000 Calorie daily food intake is left for broccoli, beans, beef, etc.?

Correct Answer
verified

A system initially has an internal energy E of 501 J. It undergoes a process during which it releases 111 J of heat energy to the surroundings, and does work of 222 J. What is the final energy of the system, in J?

Correct Answer
verified

The combustion of glucose (C₆H₁₂O₆) with oxygen gas produces carbon dioxide and water. This process releases 2803 kJ per mole of glucose. When 3.00 mol of oxygen react in this way with glucose, what is the energy release in kcal? (Hint: Write a balanced equation for the combustion process.)

Correct Answer
verified
B

The standard state of a substance in aqueous solution is a 1 M solution.

Correct Answer
verified

$\Delta$ H does not depend on the path of a reaction, but $\Delta$ E does.

Correct Answer
verified
False

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25 $\degree$ C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g ? K)

Correct Answer
verified

A system delivers 225 J of heat to the surroundings while delivering 645 J of work. Calculate the change in the internal energy, $\Delta$ E, of the system.

Correct Answer
verified

Correct Answer
verified

For all processes, both q and $\Delta$ E will have the same sign.

Correct Answer
verified

For a reaction in a sealed, rigid container, $\Delta$ H is always greater than $\Delta$ E.

Correct Answer
verified

Consider the equation $\Delta$ E = q + w. Explain fully the meaning of all three terms in the equation, and also the implied sign convention for q and w.

Correct Answer
verified
E is the internal energy of a system, i....
View Answer

A system that does no work but which receives heat from the surroundings has:

Correct Answer
verified

A system contracts from an initial volume of 15.0 L to a final volume of 10.0 L under a constant external pressure of 0.800 atm. The value of w, in J, is:

Correct Answer
verified

For which one of the following reactions will $\Delta$ H be approximately (or exactly) equal to $\Delta$ E?

Correct Answer
verified

Which of the following is not a state function?

Correct Answer
verified

Standard heats (enthalpies) of formation of compounds, $\Delta$ H $\degree$ _f, may be positive or negative.

Correct Answer
verified

In which of the following processes is $\Delta$ H = $\Delta$ E ?

Correct Answer
verified
C

Clearly state the thermodynamic standard state of A) an element or compound. B) a solute.

Correct Answer
verified
a. Standard state is the stabl...
View Answer

Exam 6: Thermochemistry: Energy Flow and Chemical Change

Correct AnswerverifiedTemperatur...View AnswerShow Answer

.

Correct AnswerverifiedShow Answer

Your favorite candy bar, Gummy Beakers, contains 1.2 *106 J of energy while your favorite soft drink, Bolt, contains 6.7 *105 J. If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt, what percent of your 2000 Calorie daily food intake is left for broccoli, beans, beef, etc.?

Correct AnswerverifiedShow Answer

A system initially has an internal energy E of 501 J. It undergoes a process during which it releases 111 J of heat energy to the surroundings, and does work of 222 J. What is the final energy of the system, in J?

Correct AnswerverifiedShow Answer

The combustion of glucose (C6H12O6) with oxygen gas produces carbon dioxide and water. This process releases 2803 kJ per mole of glucose. When 3.00 mol of oxygen react in this way with glucose, what is the energy release in kcal? (Hint: Write a balanced equation for the combustion process.)

Correct AnswerverifiedB

The standard state of a substance in aqueous solution is a 1 M solution.

Correct AnswerverifiedShow Answer

Δ\DeltaΔ H does not depend on the path of a reaction, but Δ\DeltaΔ E does.

Correct AnswerverifiedFalse

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25 °\degree° C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g ? K)

Correct AnswerverifiedShow Answer

A system delivers 225 J of heat to the surroundings while delivering 645 J of work. Calculate the change in the internal energy, Δ\DeltaΔ E, of the system.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For all processes, both q and Δ\DeltaΔ E will have the same sign.

Correct AnswerverifiedShow Answer

For a reaction in a sealed, rigid container, Δ\DeltaΔ H is always greater than Δ\DeltaΔ E.

Correct AnswerverifiedShow Answer

Consider the equation Δ\DeltaΔ E = q + w. Explain fully the meaning of all three terms in the equation, and also the implied sign convention for q and w.

Correct AnswerverifiedE is the internal energy of a system, i....View AnswerShow Answer

A system that does no work but which receives heat from the surroundings has:

Correct AnswerverifiedShow Answer

A system contracts from an initial volume of 15.0 L to a final volume of 10.0 L under a constant external pressure of 0.800 atm. The value of w, in J, is:

Correct AnswerverifiedShow Answer

For which one of the following reactions will Δ\DeltaΔ H be approximately (or exactly) equal to Δ\DeltaΔ E?

Correct AnswerverifiedShow Answer

Which of the following is not a state function?

Correct AnswerverifiedShow Answer

Standard heats (enthalpies) of formation of compounds, Δ\DeltaΔ H °\degree° f, may be positive or negative.

Correct AnswerverifiedShow Answer

In which of the following processes is Δ\DeltaΔ H = Δ\DeltaΔ E ?

Correct AnswerverifiedC

Clearly state the thermodynamic standard state of A) an element or compound. B) a solute.

Correct Answerverifieda. Standard state is the stabl...View AnswerShow Answer

Correct Answer
verified
Temperatur...
View Answer

Correct Answer
verified

Your favorite candy bar, Gummy Beakers, contains 1.2 10⁶ J of energy while your favorite soft drink, Bolt, contains 6.7 10⁵ J. If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt, what percent of your 2000 Calorie daily food intake is left for broccoli, beans, beef, etc.?

Correct Answer
verified

Correct Answer
verified

The combustion of glucose (C₆H₁₂O₆) with oxygen gas produces carbon dioxide and water. This process releases 2803 kJ per mole of glucose. When 3.00 mol of oxygen react in this way with glucose, what is the energy release in kcal? (Hint: Write a balanced equation for the combustion process.)

Correct Answer
verified
B

Correct Answer
verified

$\Delta$ H does not depend on the path of a reaction, but $\Delta$ E does.

Correct Answer
verified
False

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25 $\degree$ C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g ? K)

Correct Answer
verified

A system delivers 225 J of heat to the surroundings while delivering 645 J of work. Calculate the change in the internal energy, $\Delta$ E, of the system.

Correct Answer
verified

Correct Answer
verified

For all processes, both q and $\Delta$ E will have the same sign.

Correct Answer
verified

For a reaction in a sealed, rigid container, $\Delta$ H is always greater than $\Delta$ E.

Correct Answer
verified

Consider the equation $\Delta$ E = q + w. Explain fully the meaning of all three terms in the equation, and also the implied sign convention for q and w.

Correct Answer
verified
E is the internal energy of a system, i....
View Answer

Correct Answer
verified

Correct Answer
verified

For which one of the following reactions will $\Delta$ H be approximately (or exactly) equal to $\Delta$ E?

Correct Answer
verified

Correct Answer
verified

Standard heats (enthalpies) of formation of compounds, $\Delta$ H $\degree$ _f, may be positive or negative.

Correct Answer
verified

In which of the following processes is $\Delta$ H = $\Delta$ E ?

Correct Answer
verified
C

Correct Answer
verified
a. Standard state is the stabl...
View Answer