Question 1

The heat of combustion of propane, C3H8, 2220 kJ/mol.The specific heat of copper is 0.385 J/g.°C.How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings

Accepted Answer

The answer of The heat of combustion of propane, C3H8,...

Question 2

Given the thermochemical equation 2SO2 + O2  →\rarr→   2SO3,  Δ\DeltaΔ H°rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO3?

Accepted Answer

A)  198 kJ/mol
B)  -99 kJ/mol
C)  99 kJ/mol
D)  396 kJ/mol
E)  -198 kJ/mol F) A) and D)
G) B) and D)

Question 3

Find $\Delta$H°rxn for the reaction
2Ag2S(s)+ 2H2O(l)$\rarr$ 4Ag(s)+ 2H2S(g)+ O2(g).
[$\Delta$H°f (Ag2S(s))= -32.6 kJ/mol; $\Delta$H°f (H2S(g))= -20.5 kJ/mol; $\Delta$H°f (H2O(l))= -285.5 kJ/mol]

Accepted Answer

The answer of Find $\Delta$H°rxn for the reaction
2Ag2S(s)+ 2H2O(l)$\rarr$ 4Ag(s)+...

Question 4

The enthalpy change when a strong acid is neutralized by strong base is -56.1 kJ/mol. If 135 mL of 0.450 M HI at 23.15°C is mixed with 145 mL of 0.500 M NaOH, also at 23.15°C, what will the maximum temperature reached by the resulting solution? (Assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 J/g·°C, and that the density of the final solution is that of water.)

Accepted Answer

A)  26.06°C
B)  29.19°C
C)  32.35°C
D)  20.24°C
E)  36.57°CF) D) and E)
G) B) and E)

Question 5

The heat of solution of KCl is 17.2 kJ/mol and the lattice energy of KCl(s) is 701.2 kJ/mol.Calculate the total heat of hydration of 1 mol of gas phase K+ ions and Cl- ions.

Accepted Answer

A)  718 kJ
B)  684 kJ
C)  -684 kJ
D)  -718 kJ
E)  None of these.F) None of the above
G) A) and B)

Question 6

If 2Mg(s)+ O2(g)$\rarr$2MgO(s), $\Delta$H° = -1203.6 kJ/mol.
For Mg(s)+ (1/2)O2(g)$\rarr$MgO(s), the enthalpy change is $\Delta$H = -601.8 kJ/mol.

Accepted Answer

A) True 
 B)False

Question 7

Given that CaO(s) + H2O(l)  →\rarr→ Ca(OH) 2(s) ,  Δ\DeltaΔ H°rxn = -64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

Accepted Answer

A)  6.92 g
B)  56.1 g
C)  455 g
D)  606 g
E)  3.40 * 104 g F) None of the above
G) B) and D)

Question 8

The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

Accepted Answer

The answer of The specific heat of silver is 0.235...

Question 9

Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter.The heat of combustion of naphthalene is -40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000.g of water, a temperature rise of 4.21°C was observed. What is the heat capacity of the bomb calorimeter excluding the water?

Accepted Answer

A)  32.9 kJ/°C
B)  7.8 kJ/°C
C)  3.64 kJ/°C
D)  1.76 kJ/°C
E)  15.3 kJ/°CF) A) and E)
G) C) and D)

Question 10

Given 2Al(s) + (3/2) O2(g)  →\rarr→  Al2O3(s) ,  Δ\DeltaΔ H°f = -1,670 kJ/mol for Al2O3 (s) . Determine  Δ\DeltaΔ H° for the reaction 2Al2O3(s)  →\rarr→   4Al(s) + 3O2(g) .

Accepted Answer

A)  3,340 kJ/mol
B)  1,670 kJ/mol
C)  -3,340 kJ/mol
D)  -1,670 kJ/mol
E)  -835 kJ/mol F) A) and E)
G) A) and D)

Question 11

A home aquarium is an example of an open system.

Accepted Answer

A) True 
 B)False

Question 12

Potential energy is

Accepted Answer

A)  the energy stored within the structural units of chemical substances.
B)  the energy associated with the random motion of atoms and molecules.
C)  solar energy, i.e.energy that comes from the sun.
D)  energy available by virtue of an object's position.E) B) and C)
F) A) and D)

Question 13

A feverish student weighing 75 kilograms was immersed in 400.kg of water at 4.0°C to try to reduce the fever.The student's body temperature dropped from 40.0°C to 37.0°C.Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

Accepted Answer

The answer of A feverish student weighing 75 kilograms was...

Question 14

The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g)  →\rarr→ 8CO2(g) + 10H2O(l)  Δ\DeltaΔ H°rxn = -5,314 kJ/mol
What is the heat of combustion per gram of butane?

Accepted Answer

A)  -32.5 kJ/g
B)  -45.7 kJ/g
C)  -91.5 kJ/g
D)  -2,656 kJ/g
E)  -15,440 kJ/g F) B) and D)
G) A) and C)

Question 15

A 0.3423 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.000 kg of water contained therein rose from 20.22°C to 22.82°C. The heat capacity of the calorimeter is 2.21 kJ/°C.The heat capacity of water = 4.184 J/g·°C. What is the heat of combustion, in megajoules (MJ), per mole of pentane?

Accepted Answer

Question 16

Calculate the amount of work done, in joules, when 2.5 mole of H2O vaporizes at 1.0 atm and 25°C.Assume the volume of liquid H2O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

Accepted Answer

A)  6,190 kJ
B)  6.19 kJ
C)  61.1 J
D)  5.66 kJ
E)  518 JF) A) and B)
G) D) and E)

Question 17

When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000.g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is -26.42 kJ/g.

Accepted Answer

A)  15.87 kJ/°C
B)  4.18 kJ/°C
C)  5.52 kJ/°C
D)  1.34 kJ/°C
E)  752.1 kJ/°CF) All of the above
G) B) and D)

Question 18

The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 650.J/°C.)

Accepted Answer

A)  14.3°C
B)  20.8°C
C)  -7.7°C
D)  25.6°C
E)  21.4°CF) A) and B)
G) A) and D)

Question 19

The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g)  →\rarr→ 8CO2(g) + 10H2O(l)  Δ\DeltaΔ H°rxn= -5,314 kJ/mol
How many grams of CO2 are produced per 1.00 *104 kJ of heat released?

Accepted Answer

A)  23.4 g
B)  44.0 g
C)  82.3 g
D)  187 g
E)  662 g F) D) and E)
G) A) and B)

Question 20

The combustion of one mole of benzene, C6H6, in oxygen liberates 3268 kJ of heat.The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

Accepted Answer

Exam 6: Thermo-Chemistry

The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) $\Delta$ H°_rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

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Potential energy is

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A home aquarium is an example of an open system.

Correct Answer
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If 2Mg(s)+ O₂(g) $\rarr$ 2MgO(s), $\Delta$ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O₂(g) $\rarr$ MgO(s), the enthalpy change is $\Delta$ H = -601.8 kJ/mol.

Correct Answer
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A feverish student weighing 75 kilograms was immersed in 400.kg of water at 4.0°C to try to reduce the fever.The student's body temperature dropped from 40.0°C to 37.0°C.Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

Correct Answer
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The heat of combustion of propane, C₃H₈, 2220 kJ/mol.The specific heat of copper is 0.385 J/g.°C.How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings

Correct Answer
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The combustion of one mole of benzene, C₆H₆, in oxygen liberates 3268 kJ of heat.The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

Correct Answer
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Given the thermochemical equation 2SO₂ + O₂ $\rarr$ 2SO₃, $\Delta$ H°_rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO₃?

Correct Answer
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Correct Answer
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When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000.g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is -26.42 kJ/g.

Correct Answer
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The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) $\Delta$ H°_rxn= -5,314 kJ/mol How many grams of CO₂ are produced per 1.00 *10⁴ kJ of heat released?

Correct Answer
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Calculate the amount of work done, in joules, when 2.5 mole of H₂O vaporizes at 1.0 atm and 25°C.Assume the volume of liquid H₂O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

Correct Answer
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Given 2Al(s) + (3/2) O₂(g) $\rarr$ Al₂O₃(s) , $\Delta$ H°_f = -1,670 kJ/mol for Al₂O₃ (s) . Determine $\Delta$ H° for the reaction 2Al₂O₃(s) $\rarr$ 4Al(s) + 3O₂(g) .

Correct Answer
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Correct Answer
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Correct Answer
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Given that CaO(s) + H₂O(l) $\rarr$ Ca(OH) ₂(s) , $\Delta$ H°_rxn = -64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

Correct Answer
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Correct Answer
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Find $\Delta$ H°_rxn for the reaction 2Ag₂S(s)+ 2H₂O(l) $\rarr$ 4Ag(s)+ 2H₂S(g)+ O₂(g). [ $\Delta$ H°_f (Ag₂S(s))= -32.6 kJ/mol; $\Delta$ H°_f (H₂S(g))= -20.5 kJ/mol; $\Delta$ H°_f (H₂O(l))= -285.5 kJ/mol]

Correct Answer
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The heat of solution of KCl is 17.2 kJ/mol and the lattice energy of KCl(s) is 701.2 kJ/mol.Calculate the total heat of hydration of 1 mol of gas phase K⁺ ions and Cl^- ions.

Correct Answer
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The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

Correct Answer
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Exam 6: Thermo-Chemistry

The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g) →\rarr→ 8CO2(g) + 10H2O(l) Δ\DeltaΔ H°rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

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Potential energy is

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A home aquarium is an example of an open system.

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If 2Mg(s)+ O2(g) →\rarr→ 2MgO(s), Δ\DeltaΔ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O2(g) →\rarr→ MgO(s), the enthalpy change is Δ\DeltaΔ H = -601.8 kJ/mol.

Correct AnswerverifiedShow Answer

A feverish student weighing 75 kilograms was immersed in 400.kg of water at 4.0°C to try to reduce the fever.The student's body temperature dropped from 40.0°C to 37.0°C.Assuming the specific heat of the student to be 3.77 J/g·°C, what was the final temperature of the water?

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The heat of combustion of propane, C3H8, 2220 kJ/mol.The specific heat of copper is 0.385 J/g.°C.How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings

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The combustion of one mole of benzene, C6H6, in oxygen liberates 3268 kJ of heat.The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

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Given the thermochemical equation 2SO2 + O2 →\rarr→ 2SO3, Δ\DeltaΔ H°rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO3?

Correct AnswerverifiedShow Answer

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When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000.g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is -26.42 kJ/g.

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The combustion of butane produces heat according to the equation 2C4H10(g) + 13O2(g) →\rarr→ 8CO2(g) + 10H2O(l) Δ\DeltaΔ H°rxn= -5,314 kJ/mol How many grams of CO2 are produced per 1.00 *104 kJ of heat released?

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Calculate the amount of work done, in joules, when 2.5 mole of H2O vaporizes at 1.0 atm and 25°C.Assume the volume of liquid H2O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

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Given 2Al(s) + (3/2) O2(g) →\rarr→ Al2O3(s) , Δ\DeltaΔ H°f = -1,670 kJ/mol for Al2O3 (s) . Determine Δ\DeltaΔ H° for the reaction 2Al2O3(s) →\rarr→ 4Al(s) + 3O2(g) .

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Given that CaO(s) + H2O(l) →\rarr→ Ca(OH) 2(s) , Δ\DeltaΔ H°rxn = -64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

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The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 650.J/°C.)

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Find Δ\DeltaΔ H°rxn for the reaction 2Ag2S(s)+ 2H2O(l) →\rarr→ 4Ag(s)+ 2H2S(g)+ O2(g). [ Δ\DeltaΔ H°f (Ag2S(s))= -32.6 kJ/mol; Δ\DeltaΔ H°f (H2S(g))= -20.5 kJ/mol; Δ\DeltaΔ H°f (H2O(l))= -285.5 kJ/mol]

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The heat of solution of KCl is 17.2 kJ/mol and the lattice energy of KCl(s) is 701.2 kJ/mol.Calculate the total heat of hydration of 1 mol of gas phase K+ ions and Cl- ions.

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The specific heat of silver is 0.235 J/g·°C. How many joules of heat are required to heat a 75 g silver spoon from 20°C to 35°C?

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The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) $\Delta$ H°_rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

Correct Answer
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Correct Answer
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Correct Answer
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If 2Mg(s)+ O₂(g) $\rarr$ 2MgO(s), $\Delta$ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O₂(g) $\rarr$ MgO(s), the enthalpy change is $\Delta$ H = -601.8 kJ/mol.

Correct Answer
verified

Correct Answer
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The heat of combustion of propane, C₃H₈, 2220 kJ/mol.The specific heat of copper is 0.385 J/g.°C.How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings

Correct Answer
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The combustion of one mole of benzene, C₆H₆, in oxygen liberates 3268 kJ of heat.The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

Correct Answer
verified

Given the thermochemical equation 2SO₂ + O₂ $\rarr$ 2SO₃, $\Delta$ H°_rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO₃?

Correct Answer
verified

Correct Answer
verified

Correct Answer
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The combustion of butane produces heat according to the equation 2C₄H₁₀(g) + 13O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) $\Delta$ H°_rxn= -5,314 kJ/mol How many grams of CO₂ are produced per 1.00 *10⁴ kJ of heat released?

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Calculate the amount of work done, in joules, when 2.5 mole of H₂O vaporizes at 1.0 atm and 25°C.Assume the volume of liquid H₂O is negligible compared to that of vapor. (1 L·atm = 101.3 J)

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Given 2Al(s) + (3/2) O₂(g) $\rarr$ Al₂O₃(s) , $\Delta$ H°_f = -1,670 kJ/mol for Al₂O₃ (s) . Determine $\Delta$ H° for the reaction 2Al₂O₃(s) $\rarr$ 4Al(s) + 3O₂(g) .

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Correct Answer
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Correct Answer
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Given that CaO(s) + H₂O(l) $\rarr$ Ca(OH) ₂(s) , $\Delta$ H°_rxn = -64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

Correct Answer
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Correct Answer
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Find $\Delta$ H°_rxn for the reaction 2Ag₂S(s)+ 2H₂O(l) $\rarr$ 4Ag(s)+ 2H₂S(g)+ O₂(g). [ $\Delta$ H°_f (Ag₂S(s))= -32.6 kJ/mol; $\Delta$ H°_f (H₂S(g))= -20.5 kJ/mol; $\Delta$ H°_f (H₂O(l))= -285.5 kJ/mol]

Correct Answer
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The heat of solution of KCl is 17.2 kJ/mol and the lattice energy of KCl(s) is 701.2 kJ/mol.Calculate the total heat of hydration of 1 mol of gas phase K⁺ ions and Cl^- ions.

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Correct Answer
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