Question 1

Identify the major greenhouse gas.

Accepted Answer

A)  CO2 
B)  O2 
C)  CO 
D)  NO 
E)  NO2 
A)  CO2 
B)  O2 
C)  CO 
D)  NO 
E)  NO2

Question 2

A 6.00 g sample of copper metal at 25.0 °C is heated by the addition of 97.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is

Accepted Answer

A)  26.5 
B)  98.5 
C)  42.5 
D)  17.5 
E)  67.5 
A)  26.5 
B)  98.5 
C)  42.5 
D)  17.5 
E)  67.5

Question 3

Astatine is an extremely rare element with an estimated 28 g total on Earth. How much energy would be required to heat Earth's entire supply of astatine by 10.0 °C assuming it has a specific heat capacity similar to iodine, 0.214 J g-1 °C-1?

Accepted Answer

A)  60 J 
B)  24 J 
C)  130 J 
D)  14 J 
E)  250 J 
A)  60 J 
B)  24 J 
C)  130 J 
D)  14 J 
E)  250 J

Question 4

Which of the following statements is TRUE?

Accepted Answer

A)  Enthalpy is a state function. 
B)  An endothermic reaction has a negative enthalpy. 
C)  An exothermic reaction has a positive enthalpy. 
D)  Enthalpy change is zero under constant pressure. 
E)  The magnitude of enthalpy change is always positive. 
A)  Enthalpy is a state function. 
B)  An endothermic reaction has a negative enthalpy. 
C)  An exothermic reaction has a positive enthalpy. 
D)  Enthalpy change is zero under constant pressure. 
E)  The magnitude of enthalpy change is always positive.

Question 5

Two solutions, initially at 24.69 °C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J °C-1). When a 200.0 mL volume of 0.100 mol L-1 AgNO3 solution is mixed with a 100.0 mL sample of 0.100 mol L-1 NaCl solution, the temperature in the calorimeter rises to 25.16 °C. Determine the   H°, in units of kJ   . Assume that the density and heat capacity of the solutions is the same as that of water. Hint: Write a balanced reaction for the process.

Accepted Answer

A)  -32 kJ mol-1 
B)  -78 kJ mol-1 
C)  -64 kJ mol-1 
D)  -25 kJ mol-1 
E)  -52 kJ mol-1 
A)  -32 kJ mol-1 
B)  -78 kJ mol-1 
C)  -64 kJ mol-1 
D)  -25 kJ mol-1 
E)  -52 kJ mol-1

Question 6

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g-1 °C-1) that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

Accepted Answer

A)  3.15 °C 
B)  0.941 °C 
C)  -13.5 °C 
D)  8.49 °C 
E)  5.23 °C 
A)  3.15 °C 
B)  0.941 °C 
C)  -13.5 °C 
D)  8.49 °C 
E)  5.23 °C

Question 7

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Accepted Answer

A)  4.38 J   °C-1 
B)  2.29 J   °C-1 
C)  3.95 J   °C-1 
D)  2.53 J   °C-1 
E)  1.87 J   °C-1 
A)  4.38 J   °C-1 
B)  2.29 J   °C-1 
C)  3.95 J   °C-1 
D)  2.53 J   °C-1 
E)  1.87 J   °C-1

Question 8

________ is a piece of equipment designed to measurechange in internal energy for combustion reactions.

Accepted Answer

A)  Coffee cup calorimeter 
B)  Bomb calorimeter 
C)  Thermal calorimeter 
D)  Power compensation calorimeter 
E)  Isothermal calorimeter 
A)  Coffee cup calorimeter 
B)  Bomb calorimeter 
C)  Thermal calorimeter 
D)  Power compensation calorimeter 
E)  Isothermal calorimeter

Question 9

Calculate the change in internal energy (ΔU) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 bar. (Remember that 100 J = 1 L bar)

Accepted Answer

A)  +51.8 kJ 
B)  -15.8 kJ 
C)  -16.6 kJ 
D)  -29.3 kJ 
E)  +34.2 kJ 
A)  +51.8 kJ 
B)  -15.8 kJ 
C)  -16.6 kJ 
D)  -29.3 kJ 
E)  +34.2 kJ

Question 10

Match the following.
-+w

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 11

How much energy is evolved during the reaction of 48.7 g of Al according to the reaction below? Assume that there is excess 
Fe2O3. Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s)   H° = -852 kJ

Accepted Answer

A)  415 kJ 
B)  207 kJ 
C)  241 kJ 
D)  130 kJ 
E)  769 kJ 
A)  415 kJ 
B)  207 kJ 
C)  241 kJ 
D)  130 kJ 
E)  769 kJ

Question 12

What volume of benzene (C6H6, d = 0.88 g mL-1, molar mass = 78.11 g mol-1) is required to produce 1.5 × 103 kJ of heat according to the following reaction? 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g)   H° = -6278 kJ

Accepted Answer

A)  75 mL 
B)  37 mL 
C)  21 mL 
D)  19 mL 
E)  42 mL 
A)  75 mL 
B)  37 mL 
C)  21 mL 
D)  19 mL 
E)  42 mL

Question 13

Calculate the initial temperature of 21.8 g of lithium (specific heat capacity = 3.582 J g-1 °C-1) that absorbs 1642 J of energy from the surroundings and has a final temperature of 31.08 °C.

Accepted Answer

A)  52.11 °C 
B)  38.04 °C 
C)  26.74 °C 
D)  10.05 °C 
E)  3.17 °C 
A)  52.11 °C 
B)  38.04 °C 
C)  26.74 °C 
D)  10.05 °C 
E)  3.17 °C

Question 14

Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat?

Accepted Answer

A)  10.0 g Ag, CAg = 0.235 J g-1 °C-1 
B)  10.0 g H2O,   = 4.184 J g-1 °C-1 
C)  10.0 g ethanol, Cethanol = 2.42 J g-1 °C-1 
D)  10.0 g Fe, CFe = 0.449 J g-1 °C-1 
E)  10.0 g Au, CAu = 0.128 J g-1 °C-1 
A)  10.0 g Ag, CAg = 0.235 J g-1 °C-1 
B)  10.0 g H2O,   = 4.184 J g-1 °C-1 
C)  10.0 g ethanol, Cethanol = 2.42 J g-1 °C-1 
D)  10.0 g Fe, CFe = 0.449 J g-1 °C-1 
E)  10.0 g Au, CAu = 0.128 J g-1 °C-1

Question 15

Which of the following is in a non-standard state?

Accepted Answer

A)  a solid at 25 °F 
B)  a liquid at 25 °C 
C)  a solution at 1 bar 
D)  a solution at 1 mol L-1 
E)  a liquid at 1 bar 
A)  a solid at 25 °F 
B)  a liquid at 25 °C 
C)  a solution at 1 bar 
D)  a solution at 1 mol L-1 
E)  a liquid at 1 bar

Question 16

Which of the following is TRUE if   U = -95 J?

Accepted Answer

A)  The system is gaining 95 J, while the surroundings are losing 95 J. 
B)  The system is losing 95 J, while the surroundings are gaining 95 J. 
C)  Both the system and the surroundings are gaining 95 J. 
D)  Both the system and the surroundings are losing 95 J. 
E)  None of the above are true. 
A)  The system is gaining 95 J, while the surroundings are losing 95 J. 
B)  The system is losing 95 J, while the surroundings are gaining 95 J. 
C)  Both the system and the surroundings are gaining 95 J. 
D)  Both the system and the surroundings are losing 95 J. 
E)  None of the above are true.

Question 17

Use the standard reaction enthalpies given below to determine   H° for the following reaction: 4SO3(g) → 4S(s) + 6O2(g)   H° = ?
Given:
SO2(g) → S(s) + O2(g)   H° = +296.8 kJ
2SO2(g) + O2(g) → 2SO3(g)   H° = -197.8 kJ

Accepted Answer

A)  -494.6 kJ mol-1 
B)  -692.4 kJ mol-1 
C)  -791.4 kJ mol-1 
D)  1583 kJ mol-1 
E)  -293.0 kJ mol-1 
A)  -494.6 kJ mol-1 
B)  -692.4 kJ mol-1 
C)  -791.4 kJ mol-1 
D)  1583 kJ mol-1 
E)  -293.0 kJ mol-1

Question 18

An unknown metal alloy, specific heat capacity = 0.372 J g-1 °C-1, has a temperature change of +21.7 °C after a heat transfer of 216.4 J. Calculate the mass of the alloy in question.

Accepted Answer

A)  14.8 g 
B)  19.0 g 
C)  36.2 g 
D)  21.5 g 
E)  26.8 g 
A)  14.8 g 
B)  19.0 g 
C)  36.2 g 
D)  21.5 g 
E)  26.8 g

Question 19

Calculate the final temperature of 82.1 g of molecular hydrogen (specific heat capacity = 14.304 J g-1 °C-1) initially at 5.48 °C that absorbs 57 kJ of energy from the surroundings.

Accepted Answer

A)  14 °C 
B)  24 °C 
C)  34 °C 
D)  44 °C 
E)  54 °C 
A)  14 °C 
B)  24 °C 
C)  34 °C 
D)  44 °C 
E)  54 °C

Question 20

Use the information provided to determine   H° for the following reaction: CH4(g) + 3Cl2(g) → CHCl3(l) + 3HCl(g) H° = ?   H° (kJ   )
CH4(g) -75
CHCl3(l) -134
HCl(g) -92

Accepted Answer

A)  -151 kJ mol-1 
B)  -335 kJ mol-1 
C)  +662 kJ mol-1 
D)  +117 kJ mol-1 
E)  -217 kJ mol-1 
A)  -151 kJ mol-1 
B)  -335 kJ mol-1 
C)  +662 kJ mol-1 
D)  +117 kJ mol-1 
E)  -217 kJ mol-1

Exam 6: Thermochemistry

Identify the major greenhouse gas.

A 6.00 g sample of copper metal at 25.0 °C is heated by the addition of 97.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is

Astatine is an extremely rare element with an estimated 28 g total on Earth. How much energy would be required to heat Earth's entire supply of astatine by 10.0 °C assuming it has a specific heat capacity similar to iodine, 0.214 J g-1 °C-1?

Which of the following statements is TRUE?

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g-1 °C-1) that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

________ is a piece of equipment designed to measurechange in internal energy for combustion reactions.

Calculate the change in internal energy (ΔU) for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 24.0 L in volume at 1.00 bar. (Remember that 100 J = 1 L bar)

Match the following. -+w

How much energy is evolved during the reaction of 48.7 g of Al according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s) H° = -852 kJ

What volume of benzene (C6H6, d = 0.88 g mL-1, molar mass = 78.11 g mol-1) is required to produce 1.5 × 103 kJ of heat according to the following reaction? 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) H° = -6278 kJ

Calculate the initial temperature of 21.8 g of lithium (specific heat capacity = 3.582 J g-1 °C-1) that absorbs 1642 J of energy from the surroundings and has a final temperature of 31.08 °C.

Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat?

Which of the following is in a non-standard state?

Which of the following is TRUE if U = -95 J?

Use the standard reaction enthalpies given below to determine H° for the following reaction: 4SO3(g) → 4S(s) + 6O2(g) H° = ? Given: SO2(g) → S(s) + O2(g) H° = +296.8 kJ 2SO2(g) + O2(g) → 2SO3(g) H° = -197.8 kJ

An unknown metal alloy, specific heat capacity = 0.372 J g-1 °C-1, has a temperature change of +21.7 °C after a heat transfer of 216.4 J. Calculate the mass of the alloy in question.

Calculate the final temperature of 82.1 g of molecular hydrogen (specific heat capacity = 14.304 J g-1 °C-1) initially at 5.48 °C that absorbs 57 kJ of energy from the surroundings.

Use the information provided to determine H° for the following reaction: CH4(g) + 3Cl2(g) → CHCl3(l) + 3HCl(g) H° = ? H° (kJ ) CH4(g) -75 CHCl3(l) -134 HCl(g) -92

Units of Measurement for Physical and Chemical Change

Atoms and Elements

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

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Astatine is an extremely rare element with an estimated 28 g total on Earth. How much energy would be required to heat Earth's entire supply of astatine by 10.0 °C assuming it has a specific heat capacity similar to iodine, 0.214 J g^-1 °C^-1?

Calculate the initial temperature of 448 g of grapes (specific heat capacity = 1.76 J g^-1 °C^-1) that absorb 17472 J of heat while warming up to room temperature, 23.1 °C.

How much energy is evolved during the reaction of 48.7 g of Al according to the reaction below? Assume that there is excess Fe₂O₃. Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s) H°= -852 kJ

What volume of benzene (C₆H₆, d = 0.88 g mL^-1, molar mass = 78.11 g mol^-1) is required to produce 1.5 × 10³ kJ of heat according to the following reaction? 2C₆H₆(l) + 15O₂(g) → 12CO₂(g) + 6H₂O(g) H°= -6278 kJ

Calculate the initial temperature of 21.8 g of lithium (specific heat capacity = 3.582 J g^-1 °C^-1) that absorbs 1642 J of energy from the surroundings and has a final temperature of 31.08 °C.

Use the standard reaction enthalpies given below to determine H° for the following reaction: 4SO₃(g) → 4S(s) + 6O₂(g) H°= ? Given: SO₂(g) → S(s) + O₂(g) H°= +296.8 kJ 2SO₂(g) + O₂(g) → 2SO₃(g) H°= -197.8 kJ

An unknown metal alloy, specific heat capacity = 0.372 J g^-1 °C^-1, has a temperature change of +21.7 °C after a heat transfer of 216.4 J. Calculate the mass of the alloy in question.

Calculate the final temperature of 82.1 g of molecular hydrogen (specific heat capacity = 14.304 J g^-1 °C^-1) initially at 5.48 °C that absorbs 57 kJ of energy from the surroundings.

Use the information provided to determine H° for the following reaction: CH₄(g) + 3Cl₂(g) → CHCl₃(l) + 3HCl(g) H°= ? H° (kJ ) CH₄(g) -75 CHCl₃(l) -134 HCl(g) -92