Question 1

Identify the unit of specific heat capacity.

Accepted Answer

A)  °C-1 
B)  J g-1 °C-1 
C)  J mol-1 °C-1 
D)  g °C-1 
E)  mol °C-1 
A)  °C-1 
B)  J g-1 °C-1 
C)  J mol-1 °C-1 
D)  g °C-1 
E)  mol °C-1

Question 2

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g   . B2H6(g) + 6Cl2(g) → 2BCl3(g) + 6HCl(g)   H° = -1396 kJ

Accepted Answer

A)  1640 kJ 
B)  238 kJ 
C)  1430 kJ 
D)  3070 kJ 
E)  429 kJ 
A)  1640 kJ 
B)  238 kJ 
C)  1430 kJ 
D)  3070 kJ 
E)  429 kJ

Question 3

A 5.00 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)  25.9 
B)  146 
C)  6.93 
D)  -18.1 
E)  31.9 
A)  25.9 
B)  146 
C)  6.93 
D)  -18.1 
E)  31.9

Question 4

Give the temperature and pressure for the standard state for a liquid.

Accepted Answer

For the standard state of liqu

Question 5

Calculate the heat transfer, in kJ, when 1.287 kg of chicken breast (specific heat capacity = 1.82 J g-1 °C-1) is removed from a freezer at -17.3 °C and allowed to warm up to 0.00 °C. You need not be concerned about melting of ice or any other phase changes.

Accepted Answer

A)  -0.0405 kJ 
B)  0.0405 kJ 
C)  -40.5 kJ 
D)  40.5 kJ 
E)  8.65 kJ 
A)  -0.0405 kJ 
B)  0.0405 kJ 
C)  -40.5 kJ 
D)  40.5 kJ 
E)  8.65 kJ

Question 6

A 12.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity of 5.65 kJ   . Using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°C. The molar mass of ethanol is 46.07 g   . C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g)   U = -1235 kJ

Accepted Answer

A)  53.4 °C 
B)  28.1 °C 
C)  111 °C 
D)  85.7 °C 
E)  74.2 °C 
A)  53.4 °C 
B)  28.1 °C 
C)  111 °C 
D)  85.7 °C 
E)  74.2 °C

Question 7

Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g mol-1. The molar mass of carbon dioxide is 44.0095 g mol-1. 2C8H18 + 25O2 → 16CO2 + 18H2O   H° = -11018 kJ

Accepted Answer

A)  800.1 g 
B)  307.9 g 
C)  260.1 g 
D)  792.3 g 
A)  800.1 g 
B)  307.9 g 
C)  260.1 g 
D)  792.3 g

Question 8

Define heat capacity.

Accepted Answer

A)  the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C 
B)  the quantity of heat required to change a system's temperature by 1 °C 
C)  the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C 
D)  the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F 
E)  the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C 
A)  the quantity of heat required to raise the temperature of 1 mol of a substance by 1 °C 
B)  the quantity of heat required to change a system's temperature by 1 °C 
C)  the quantity of heat required to raise the temperature of 1 g of a substance by 1 °C 
D)  the quantity of heat required to raise the temperature of 1 g of a substance by 1 °F 
E)  the quantity of heat required to raise the temperature of 1 L of a substance by 1 °C

Question 9

In the presence of excess oxygen, methane gas burns in a constant pressure system to yield carbon dioxide and water:   (g) +   (g) →   (g) +   O (l)   H = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure.

Accepted Answer

A)  -0.00946 kJ   
B)  0.0342 kJ   
C)  -1.06 ×   kJ   
D)  29.3 kJ   
E)  -106 kJ   
A)  -0.00946 kJ   
B)  0.0342 kJ   
C)  -1.06 ×   kJ   
D)  29.3 kJ   
E)  -106 kJ

Question 10

Calculate the initial temperature of 648 g of cucumber (specific heat capacity = 1.88 J g-1 °C-1) that absorbs 19857 J of heat while warming up to room temperature, 24.8 °C.

Accepted Answer

A)  9.62 °C 
B)  8.50 °C 
C)  10.3 °C 
D)  14.8 °C 
E)  3.41 °C 
A)  9.62 °C 
B)  8.50 °C 
C)  10.3 °C 
D)  14.8 °C 
E)  3.41 °C

Question 11

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)    U can be determined using constant volume calorimetry. 
C)  Energy is neither created nor destroyed, excluding nuclear reactions. 
D)    H 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)    U can be determined using constant volume calorimetry. 
C)  Energy is neither created nor destroyed, excluding nuclear reactions. 
D)    H can be determined using constant pressure calorimetry. 
E)  All of the above are true.

Question 12

A 2.38 g sample of phenol (C6H6O, molar mass = 94.11 g   ) was combusted in a bomb calorimeter with a heat capacity of 6.65 kJ   . If the temperature increased from 23.8 °C to 35.4 °C, determine   U for the combustion of phenol.

Accepted Answer

A)  -8.19 × 103 kJ mol-1 
B)  -5.81 × 103 kJ mol-1 
C)  4.87 × 103 kJ mol-1 
D)  -3.05 × 103 kJ mol-1 
E)  2.41 × 103 kJ mol-1 
A)  -8.19 × 103 kJ mol-1 
B)  -5.81 × 103 kJ mol-1 
C)  4.87 × 103 kJ mol-1 
D)  -3.05 × 103 kJ mol-1 
E)  2.41 × 103 kJ mol-1

Question 13

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

Accepted Answer

A)  50.0 g Al, CAl = 0.903 J g-1 °C-1 
B)  50.0 g Cu, CCu = 0.385 J g-1 °C-1 
C)  25.0 g granite, Cgranite = 0.79 J g-1 °C-1 
D)  25.0 g Au, CAu = 0.128 J g-1 °C-1 
E)  25.0 g Ag, CAg = 0.235 J g-1 °C-1 
A)  50.0 g Al, CAl = 0.903 J g-1 °C-1 
B)  50.0 g Cu, CCu = 0.385 J g-1 °C-1 
C)  25.0 g granite, Cgranite = 0.79 J g-1 °C-1 
D)  25.0 g Au, CAu = 0.128 J g-1 °C-1 
E)  25.0 g Ag, CAg = 0.235 J g-1 °C-1

Question 14

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, ΔcombustionU = -15.48 kJ g-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of Ccal?

Accepted Answer

A)  24.34 kJ °C-1 
B)  8.009 kJ °C-1 
C)  14.18 kJ °C-1 
D)  16.67 kJ °C-1 
E)  9.170 kJ °C-1 
A)  24.34 kJ °C-1 
B)  8.009 kJ °C-1 
C)  14.18 kJ °C-1 
D)  16.67 kJ °C-1 
E)  9.170 kJ °C-1

Question 15

8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then ________.

Accepted Answer

A)  ΔH° = +546.4 kJ and ΔU° = +576.06 kJ 
B)  ΔH° = +546.4 kJ and ΔU° = +516.8 kJ 
C)  ΔH° = -546.4 kJ and ΔU° = -516.8 kJ 
D)  ΔH° = -546.4 kJ and ΔU° = -576.0 kJ 
A)  ΔH° = +546.4 kJ and ΔU° = +576.06 kJ 
B)  ΔH° = +546.4 kJ and ΔU° = +516.8 kJ 
C)  ΔH° = -546.4 kJ and ΔU° = -516.8 kJ 
D)  ΔH° = -546.4 kJ and ΔU° = -576.0 kJ

Question 16

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-1 °C-1.

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

Question 17

Choose the reaction that illustrates ΔH° for NaHCO3.

Accepted Answer

A)  Na(s) + H2(g) + C(s) + O2(g) → NaHCO3 (s) 
B)  Na+(aq) + HCO3 -1 (aq) → NaHCO3 (s) 
C)  Na+(aq) + H2O (l) + CO2 (g) → NaHCO3(s) 
D)  Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) → NaHCO3 (s) 
E)  Na(s) + 2 H(g) + C(s) + 3 O(g) → NaHCO3(s) 
A)  Na(s) + H2(g) + C(s) + O2(g) → NaHCO3 (s) 
B)  Na+(aq) + HCO3 -1 (aq) → NaHCO3 (s) 
C)  Na+(aq) + H2O (l) + CO2 (g) → NaHCO3(s) 
D)  Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) → NaHCO3 (s) 
E)  Na(s) + 2 H(g) + C(s) + 3 O(g) → NaHCO3(s)

Question 18

A student is preparing to perform a series of calorimetry experiments. She first wishes to determine the calorimeter constant (Ccal) for her coffee cup calorimeter. She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K. She carefully records the final temperature of the water as 317 K. What is the value of Ccal for the calorimeter?

Accepted Answer

A)  19 J K-1 
B)  28 J K-1 
C)  99 J K-1 
D)  21 J K-1 
E)  76 J K-1 
A)  19 J K-1 
B)  28 J K-1 
C)  99 J K-1 
D)  21 J K-1 
E)  76 J K-1

Question 19

Match the following.
-+ q

Accepted Answer

A) energy flows out of the system into the surroundings 
B) energy flows into the system from the surroundings 
C) work done by the system on the surroundings 
D) the system loses thermal energy to the surroundings 
E) the system gains thermal energy from the surroundings
F)work done on the system by the surroundings 
A) energy flows out of the system into the surroundings 
B) energy flows into the system from the surroundings 
C) work done by the system on the surroundings 
D) the system loses thermal energy to the surroundings 
E) the system gains thermal energy from the surroundings
F)work done on the system by the surroundings

Question 20

For a process at constant pressure, 62,000 calories of heat are absorbed. This quantity of heat is equivalent to ________.

Accepted Answer

A)  3.85 × 10-6 J 
B)  1.48 × 104 J 
C)  6.21 × 104 J 
D)  2.59 × 105 J 
A)  3.85 × 10-6 J 
B)  1.48 × 104 J 
C)  6.21 × 104 J 
D)  2.59 × 105 J

Exam 6: Thermochemistry

Identify the unit of specific heat capacity.

According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g . B2H6(g) + 6Cl2(g) → 2BCl3(g) + 6HCl(g) H° = -1396 kJ

A 5.00 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

Give the temperature and pressure for the standard state for a liquid.

Calculate the heat transfer, in kJ, when 1.287 kg of chicken breast (specific heat capacity = 1.82 J g-1 °C-1) is removed from a freezer at -17.3 °C and allowed to warm up to 0.00 °C. You need not be concerned about melting of ice or any other phase changes.

Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g mol-1. The molar mass of carbon dioxide is 44.0095 g mol-1. 2C8H18 + 25O2 → 16CO2 + 18H2O H° = -11018 kJ

Define heat capacity.

In the presence of excess oxygen, methane gas burns in a constant pressure system to yield carbon dioxide and water: (g) + (g) → (g) + O (l) H = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure.

Calculate the initial temperature of 648 g of cucumber (specific heat capacity = 1.88 J g-1 °C-1) that absorbs 19857 J of heat while warming up to room temperature, 24.8 °C.

Which of the following statements is TRUE?

A 2.38 g sample of phenol (C6H6O, molar mass = 94.11 g ) was combusted in a bomb calorimeter with a heat capacity of 6.65 kJ . If the temperature increased from 23.8 °C to 35.4 °C, determine U for the combustion of phenol.

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, ΔcombustionU = -15.48 kJ g-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of Ccal?

8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then ________.

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-1 °C-1.

Choose the reaction that illustrates ΔH° for NaHCO3.

Match the following. -+ q

For a process at constant pressure, 62,000 calories of heat are absorbed. This quantity of heat is equivalent to ________.

Units of Measurement for Physical and Chemical Change

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Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

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, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

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Organic Chemistry I: Structures

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According to the following reaction, how much energy is evolved during the reaction of 32.5 g B₂H₆ and 72.5 g Cl₂? The molar mass of B₂H₆is 27.67 g . B₂H₆(g) + 6Cl₂(g) → 2BCl₃(g) + 6HCl(g) H°= -1396 kJ

Calculate the heat transfer, in kJ, when 1.287 kg of chicken breast (specific heat capacity = 1.82 J g^-1 °C^-1) is removed from a freezer at -17.3 °C and allowed to warm up to 0.00 °C. You need not be concerned about melting of ice or any other phase changes.

Using the following equation for the combustion of octane, calculate the amount of grams of carbon dioxide formed from 100.0 g of octane. The molar mass of octane is 114.33 g mol^-1. The molar mass of carbon dioxide is 44.0095 g mol^-1. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O H°= -11018 kJ

Calculate the initial temperature of 648 g of cucumber (specific heat capacity = 1.88 J g^-1 °C^-1) that absorbs 19857 J of heat while warming up to room temperature, 24.8 °C.

A 2.38 g sample of phenol (C₆H₆O, molar mass = 94.11 g ) was combusted in a bomb calorimeter with a heat capacity of 6.65 kJ . If the temperature increased from 23.8 °C to 35.4 °C, determine U for the combustion of phenol.

A chemist wishes to calibrate a bomb calorimeter, so he combusts 7.529 g of D-galactose, Δ_combustionU = -15.48 kJ g^-1, which causes a temperature change from 26.38 °C to 34.60 °C. What should the chemist report for the value of C_cal?

8.000 moles of H₂(g) reacts with 4.000 mol of O₂(g) to form 8.000 mol of H₂O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then ________.

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^-1 °C^-1.

Choose the reaction that illustrates ΔH° for NaHCO₃.