The standard enthalpy of formation of NH4Cl(s) is -315.4 kJ/mol. The equation that describes this △H°f is:

A) NH4+(aq) + Cl-(aq) → NH4Cl(s) B) 1/2 N2(g) + 2H2(g) + 1/2 Cl2(g) → NH4Cl(s) C) N2(g) + H2(g) + Cl2(g) → 2 NH4Cl(s) D) 1/2 N2(g) + 1/2 Cl2(g) + 1/2 H2(g) → NH4Cl(s) E) N2(g) + Cl2(g) + 4 H2(g) → 2 NH4Cl(s) A) NH4+(aq) + Cl-(aq) → NH4Cl(s) B) 1/2 N2(g) + 2H2(g) + 1/2 Cl2(g) → NH4Cl(s) C) N2(g) + H2(g) + Cl2(g) → 2 NH4Cl(s) D) 1/2 N2(g) + 1/2 Cl2(g) + 1/2 H2(g) → NH4Cl(s) E) N2(g) + Cl2(g) + 4 H2(g) → 2 NH4Cl(s)

Given the heat of formation of the following compounds: CO2(g)&emsp; &emsp;ΔH°f = -393.5 kJ/mol H2O(l) &emsp;&emsp; ΔH°f = -285.9 kJ/mol CH3OH(l)&emsp; ΔH°f = -238.6 kJ/mol What is the value of ΔH for the reaction: CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l)

A) -440.8 kJ B) -416.9 kJ C) -1203.9 kJ D) -346.2 kJ E) -726.7 kJ A) -440.8 kJ B) -416.9 kJ C) -1203.9 kJ D) -346.2 kJ E) -726.7 kJ

500 g of Al is heated to 100.0°C and dropped into a l00.0 g glass beaker that contains 200.0 g of H2O. The temperature of the glass and water is 20.0°C. What is the final temperature? (Specific heat of Al = 0.29 J/g °C, specific heat of glass = 0.84 J/g °C)

A) 46.6 °C B) 50.0 °C C) 25.0 °C D) 30.9 °C E) 28.9 °C A) 46.6 °C B) 50.0 °C C) 25.0 °C D) 30.9 °C E) 28.9 °C

What is the reaction for the standard enthalpy of formation for Mn2O3(s)? (Mn(s) is the stable form of manganese.)

A) Mn(s) + 3/4 O2(g) → 1/2 Mn2O3(s) B) MnO(s) + MnO2(s) → Mn2O3(s) C) 2 Mn(s) + O3(g) → Mn2O3(s) D) 2 MnO(s) + 1/2 O3(g) → Mn2O3(s) E) 2Mn (s) + 3/2 O2 (g) → Mn2O3(s) A) Mn(s) + 3/4 O2(g) → 1/2 Mn2O3(s) B) MnO(s) + MnO2(s) → Mn2O3(s) C) 2 Mn(s) + O3(g) → Mn2O3(s) D) 2 MnO(s) + 1/2 O3(g) → Mn2O3(s) E) 2Mn (s) + 3/2 O2 (g) → Mn2O3(s)

Determine the enthalpy change in the following equation: Cl2(g) + H2O(l) → 2 HCl(g) + 1/2 O2(g) &emsp;&emsp;&emsp;ΔH°f H2O(l) = -285.8 kJ/mol &emsp;&emsp;&emsp;ΔH°f HCl(g) = -92.31 kJ/mol

A) 193.5 kJ B) -470.4 kJ C) 470.4 kJ D) 101.2 kJ E) -101.2 kJ A) 193.5 kJ B) -470.4 kJ C) 470.4 kJ D) 101.2 kJ E) -101.2 kJ

Consider the reaction: CO2(g) + 2HCl(g) → COCl2(g) + H2O(l) &emsp;ΔH°f -393.51 &emsp;-92.30 &emsp;-223.01 &emsp;-285.85 kJ/mol Compute ΔH° for this reaction.

A) -994.67 kJ B) 23.05 kJ C) -23.05 kJ D) 69.25 kJ E) -69.25 kJ A) -994.67 kJ B) 23.05 kJ C) -23.05 kJ D) 69.25 kJ E) -69.25 kJ

The complete combustion of propane, C3H8(g), is represented by the equation: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) &emsp; &emsp; ΔH° = -2220 kJ How much heat is evolved in the complete combustion of 12.5 L C3H8(g) at 25°C and 790 mmHg?

A) 8.27 × 104 kJ B) 1.41 × 104 kJ C) 653 kJ D) 168 kJ E) 1180 kJ A) 8.27 × 104 kJ B) 1.41 × 104 kJ C) 653 kJ D) 168 kJ E) 1180 kJ

Determine the enthalpy change in the following equation: 2/3 H2S(g) + O2(g) → 2/3 SO2(g) + 2/3 H2O(l) &emsp;&emsp;&emsp;ΔH°f H2O(l) = -285.8 kJ/mol &emsp;&emsp;&emsp;ΔH°f H2S(g) = -20.63 kJ/mol &emsp;&emsp;&emsp;ΔH°f SO2(g) = -296.8 kJ/mol

A) -562 kJ B) -375 kJ C) 375 kJ D) -402 kJ E) 402 kJ A) -562 kJ B) -375 kJ C) 375 kJ D) -402 kJ E) 402 kJ

Given the following thermochemical equations: (kJ) 4 FeS2(s) + 11O2(g) → 2 Fe2O3(s) + 8 SO2(g) ΔH° = -3307.9 2 H2S(g) + 3O2(g) → 2 H2O(l) + 2 SO2(g) - 1125.2 4 FeO(s) + O2(g) → 2 Fe2O3(s) - 578.2 2 Fe(s) + O2(g) → 2 FeO(s) - 544 H2(g) + S(rh) → H2S(g) - 20.2 2 H2(g) + O2(g) → 2 H2O(l) - 571.7 Compute the ΔH°f for FeS2(s) in kJ/mol.

A) -1233.9 kJ B) -2893.9 kJ C) -24.3 kJ D) -183.5 kJ E) -70.0 kJ A) -1233.9 kJ B) -2893.9 kJ C) -24.3 kJ D) -183.5 kJ E) -70.0 kJ

Exam 7: Thermochemistry

Many people believe that coffee (sp ht = 4.18 J/g °C) may be cooled by placing a silver spoon (sp ht = 0.237 J/g °C) in the coffee. If 250 ml (d = 1.00 g/mL) of coffee at 200°F had a spoon at 70°F placed in it, what would be the final Celsius temperature of the spoon and coffee, assuming that no heat is lost to the surroundings? The mass of the spoon is 35 g.

(Multiple Choice)

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Question 21

Calculate the standard enthalpy of formation of Cl-(aq), given the following thermochemical data at 1 atm, and knowing that the standard enthalpies of formation of H₂(g) and H⁺(aq) are both zero. HCl(g) → H⁺(aq) + Cl-(aq) -75.15 kJ H₂(g) + Cl₂(g) → 2HCl(g) -184.62 kJ

(Multiple Choice)

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Question 22

The standard enthalpy of formation of NH₄Cl(s) is -315.4 kJ/mol. The equation that describes this △H°f is:

(Multiple Choice)

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Question 23

What is the reaction for the standard enthalpy of formation for HCl(g)?

(Multiple Choice)

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Question 24

Kinetic energy is the energy of motion.

(True/False)

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Question 25

Given the heat of formation of the following compounds: CO₂(g) ΔH°f = -393.5 kJ/mol H₂O(l) ΔH°f = -285.9 kJ/mol CH₃OH(l) ΔH°f = -238.6 kJ/mol What is the value of ΔH for the reaction: CH₃OH(l) + 3/2 O₂(g) → CO₂(g) + 2 H₂O(l)

(Multiple Choice)

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Question 26

500 g of Al is heated to 100.0°C and dropped into a l00.0 g glass beaker that contains 200.0 g of H₂O. The temperature of the glass and water is 20.0°C. What is the final temperature? (Specific heat of Al = 0.29 J/g °C, specific heat of glass = 0.84 J/g °C)

(Multiple Choice)

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Question 27

Calculate the work needed to make room for products in the combustion of sulfur, S8(s), to SO₂(g) at STP.

(Multiple Choice)

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Question 28

What is the reaction for the standard enthalpy of formation for Mn₂O₃(s)? (Mn(s) is the stable form of manganese.)

(Multiple Choice)

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Question 29

How much work, in joules, is done when the pressure is suddenly released from 4.56 atm to 1.23 atm on 45.4 g of O₂at 44°C?

(Multiple Choice)

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Question 30

How much heat is required to raise the temperature of 175 g of aluminum from 21.0°C to 145°C? The specific heat of aluminum is 0.903 J g-1 °C-1.

(Multiple Choice)

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Question 31

Determine the enthalpy change in the following equation: Cl₂(g) + H₂O(l) → 2 HCl(g) + 1/2 O₂(g) ΔH°f H₂O(l) = -285.8 kJ/mol ΔH°f HCl(g) = -92.31 kJ/mol

(Multiple Choice)

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Question 32

Enthalpy is defined as:

(Multiple Choice)

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Question 33

Consider the reaction: CO₂(g) + 2HCl(g) → COCl₂(g) + H₂O(l) ΔH°f -393.51 -92.30 -223.01 -285.85 kJ/mol Compute ΔH° for this reaction.

(Multiple Choice)

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Question 34

The complete combustion of propane, C₃H₈(g), is represented by the equation: C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(l) ΔH° = -2220 kJ How much heat is evolved in the complete combustion of 12.5 L C₃H₈(g) at 25°C and 790 mmHg?

(Multiple Choice)

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Question 35

Determine the enthalpy change in the following equation: 2/3 H₂S(g) + O₂(g) → 2/3 SO₂(g) + 2/3 H₂O(l) ΔH°f H₂O(l) = -285.8 kJ/mol ΔH°f H₂S(g) = -20.63 kJ/mol ΔH°f SO₂(g) = -296.8 kJ/mol

(Multiple Choice)

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Question 36

Given the following thermochemical equations: (kJ) 4 FeS₂(s) + 11O₂(g) → 2 Fe₂O₃(s) + 8 SO₂(g) ΔH° = -3307.9 2 H₂S(g) + 3O₂(g) → 2 H₂O(l) + 2 SO₂(g) - 1125.2 4 FeO(s) + O₂(g) → 2 Fe₂O₃(s) - 578.2 2 Fe(s) + O₂(g) → 2 FeO(s) - 544 H₂(g) + S(rh) → H₂S(g) - 20.2 2 H₂(g) + O₂(g) → 2 H₂O(l) - 571.7 Compute the ΔH°f for FeS₂(s) in kJ/mol.

(Multiple Choice)

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Question 37

The enthalpy of a system is the internal energy minus work

(True/False)

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Question 38

100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0°C. The final temperature of the nickel-water mixture was 26.3°C. What is the specific heat of the nickel?

(Multiple Choice)

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Question 39

The standard enthalpy for diamond and graphite are the same value.

(True/False)

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Question 40

Showing 21 - 40 of 101

Exam 7: Thermochemistry

Calculate the standard enthalpy of formation of Cl-(aq), given the following thermochemical data at 1 atm, and knowing that the standard enthalpies of formation of H2(g) and H+(aq) are both zero. HCl(g) → H+(aq) + Cl-(aq) -75.15 kJ H2(g) + Cl2(g) → 2HCl(g) -184.62 kJ

The standard enthalpy of formation of NH4Cl(s) is -315.4 kJ/mol. The equation that describes this △H°f is:

What is the reaction for the standard enthalpy of formation for HCl(g)?

Kinetic energy is the energy of motion.

Given the heat of formation of the following compounds: CO2(g) ΔH°f = -393.5 kJ/mol H2O(l) ΔH°f = -285.9 kJ/mol CH3OH(l) ΔH°f = -238.6 kJ/mol What is the value of ΔH for the reaction: CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l)

500 g of Al is heated to 100.0°C and dropped into a l00.0 g glass beaker that contains 200.0 g of H2O. The temperature of the glass and water is 20.0°C. What is the final temperature? (Specific heat of Al = 0.29 J/g °C, specific heat of glass = 0.84 J/g °C)

Calculate the work needed to make room for products in the combustion of sulfur, S8(s), to SO2(g) at STP.

What is the reaction for the standard enthalpy of formation for Mn2O3(s)? (Mn(s) is the stable form of manganese.)

How much work, in joules, is done when the pressure is suddenly released from 4.56 atm to 1.23 atm on 45.4 g of O2 at 44°C?

How much heat is required to raise the temperature of 175 g of aluminum from 21.0°C to 145°C? The specific heat of aluminum is 0.903 J g-1 °C-1.

Determine the enthalpy change in the following equation: Cl2(g) + H2O(l) → 2 HCl(g) + 1/2 O2(g) ΔH°f H2O(l) = -285.8 kJ/mol ΔH°f HCl(g) = -92.31 kJ/mol

Enthalpy is defined as:

Consider the reaction: CO2(g) + 2HCl(g) → COCl2(g) + H2O(l) ΔH°f -393.51 -92.30 -223.01 -285.85 kJ/mol Compute ΔH° for this reaction.

The complete combustion of propane, C3H8(g), is represented by the equation: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ How much heat is evolved in the complete combustion of 12.5 L C3H8(g) at 25°C and 790 mmHg?

Determine the enthalpy change in the following equation: 2/3 H2S(g) + O2(g) → 2/3 SO2(g) + 2/3 H2O(l) ΔH°f H2O(l) = -285.8 kJ/mol ΔH°f H2S(g) = -20.63 kJ/mol ΔH°f SO2(g) = -296.8 kJ/mol

The enthalpy of a system is the internal energy minus work

100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0°C. The final temperature of the nickel-water mixture was 26.3°C. What is the specific heat of the nickel?

The standard enthalpy for diamond and graphite are the same value.

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Calculate the standard enthalpy of formation of Cl-(aq), given the following thermochemical data at 1 atm, and knowing that the standard enthalpies of formation of H₂(g) and H⁺(aq) are both zero. HCl(g) → H⁺(aq) + Cl-(aq) -75.15 kJ H₂(g) + Cl₂(g) → 2HCl(g) -184.62 kJ

The standard enthalpy of formation of NH₄Cl(s) is -315.4 kJ/mol. The equation that describes this △H°f is:

Given the heat of formation of the following compounds: CO₂(g) ΔH°f = -393.5 kJ/mol H₂O(l) ΔH°f = -285.9 kJ/mol CH₃OH(l) ΔH°f = -238.6 kJ/mol What is the value of ΔH for the reaction: CH₃OH(l) + 3/2 O₂(g) → CO₂(g) + 2 H₂O(l)

500 g of Al is heated to 100.0°C and dropped into a l00.0 g glass beaker that contains 200.0 g of H₂O. The temperature of the glass and water is 20.0°C. What is the final temperature? (Specific heat of Al = 0.29 J/g °C, specific heat of glass = 0.84 J/g °C)

Calculate the work needed to make room for products in the combustion of sulfur, S8(s), to SO₂(g) at STP.

What is the reaction for the standard enthalpy of formation for Mn₂O₃(s)? (Mn(s) is the stable form of manganese.)

How much work, in joules, is done when the pressure is suddenly released from 4.56 atm to 1.23 atm on 45.4 g of O₂at 44°C?

Determine the enthalpy change in the following equation: Cl₂(g) + H₂O(l) → 2 HCl(g) + 1/2 O₂(g) ΔH°f H₂O(l) = -285.8 kJ/mol ΔH°f HCl(g) = -92.31 kJ/mol

Consider the reaction: CO₂(g) + 2HCl(g) → COCl₂(g) + H₂O(l) ΔH°f -393.51 -92.30 -223.01 -285.85 kJ/mol Compute ΔH° for this reaction.

The complete combustion of propane, C₃H₈(g), is represented by the equation: C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(l) ΔH° = -2220 kJ How much heat is evolved in the complete combustion of 12.5 L C₃H₈(g) at 25°C and 790 mmHg?

Determine the enthalpy change in the following equation: 2/3 H₂S(g) + O₂(g) → 2/3 SO₂(g) + 2/3 H₂O(l) ΔH°f H₂O(l) = -285.8 kJ/mol ΔH°f H₂S(g) = -20.63 kJ/mol ΔH°f SO₂(g) = -296.8 kJ/mol