In the reaction below, ΔH°f is zero for ________. Ni (s) + 2CO (g) + 2PF3 (g) → Ni(CO)2(PF3)2 (l)

A) Ni (s) B) CO (g) C) F3 (g) D) Ni(CO)2(PF3)2 (l) E) both CO (g)and PF3 (g) A) Ni (s) B) CO (g) C) F3 (g) D) Ni(CO)2(PF3)2 (l) E) both CO (g)and PF3 (g)

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

A) -100.1 kJ B) 0.0324 kJ C) -0.0100 kJ D) 30.9 kJ E) -1.00 × 105 kJ A) -100.1 kJ B) 0.0324 kJ C) -0.0100 kJ D) 30.9 kJ E) -1.00 × 105 kJ

Given the data in the table below, ΔH°rxn for the reaction 3NO2 (g) + H2O (l) → 2HNO3 (aq) + NO (g) Is ________ kJ.

A) 64 B) 140 C) -140 D) -508 E) -64 A) 64 B) 140 C) -140 D) -508 E) -64

Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2H3AsO4 → Ca(H2AsO4)2 + 2H2O Is ________ kJ.

A) -744.9 B) -4519 C) -4219 D) -130.4 E) -76.4 A) -744.9 B) -4519 C) -4219 D) -130.4 E) -76.4

Exam 5: Thermochemistry

The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH₄ (g) + 3Cl₂ (g) → CHCl₃ (l) + 3HCl (g)

(Multiple Choice)

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Question 61

In the reaction below, ΔH°_f is zero for ________. Ni (s) + 2CO (g) + 2PF₃ (g) → Ni(CO)₂(PF₃)₂ (l)

(Multiple Choice)

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Question 62

The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.

(Multiple Choice)

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Question 63

For a given process at constant pressure, w is positive. This means that the process involves ________.

(Multiple Choice)

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Question 64

The value of ΔH° for the reaction below is -126 kJ. ________ kj are released when 2.00 mol of NaOH is formed in the reaction? 2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

(Multiple Choice)

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Question 65

The temperature of a 11.8 g sample of calcium carbonate [CaCO₃ (s)] increases from 24.8 °C to 38.0 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed?

(Multiple Choice)

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Question 66

Given the following reactions N₂ (g) + O₂ (g) → 2NO (g)ΔH = +180.7 kJ 2NO( g) + O₂ (g) → 2NO₂ (g)ΔH = -113.1 kJ The enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO₂ (g) → N₂ (g) + 2O₂ (g) Is ________ kJ.

(Multiple Choice)

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Question 67

For which one of the following reactions is the value of ΔH°_rxn equal to ΔH°_f for the product?

(Multiple Choice)

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Question 68

One joule equals 1 kg-m²/s².

(True/False)

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Question 69

When work is done on a system, w will be a ________ value.

(Multiple Choice)

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Question 70

Which of the following is a statement of the first law of thermodynamics?

(Multiple Choice)

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Question 71

The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 2.12-kg block of copper from 25.0 °C to 99.9 °C?

(Multiple Choice)

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Question 72

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

(Multiple Choice)

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Question 73

The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 12.6-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 °C to ________°C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.

(Multiple Choice)

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Question 74

Given the data in the table below, ΔH°_rxn for the reaction 3NO₂ (g) + H₂O (l) → 2HNO₃ (aq) + NO (g) Is ________ kJ.

(Multiple Choice)

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Question 75

Given the data in the table below, ΔH°_rxn for the reaction Ca(OH)₂ + 2H₃AsO₄ → Ca(H₂AsO₄)₂ + 2H₂O Is ________ kJ.

(Multiple Choice)

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Question 76

The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________ kcal.

(Multiple Choice)

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Question 77

Calculate the work (kJ)done during a reaction in which the internal volume expands from 14 L to 50 L against a vacuum (an outside pressure of 0 atm).

(Multiple Choice)

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Question 78

The energy released by combustion of 1 g of a substance is called the ________ of the substance.

(Multiple Choice)

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Question 79

The standard enthalpy change of a reaction is the enthalpy change when all reactants and products are at ________ pressure and a specific temperature.

(Short Answer)

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Question 80

Showing 61 - 80 of 154

Exam 5: Thermochemistry

The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH4 (g) + 3Cl2 (g) → CHCl3 (l) + 3HCl (g)

In the reaction below, ΔH°f is zero for ________. Ni (s) + 2CO (g) + 2PF3 (g) → Ni(CO)2(PF3)2 (l)

The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is ________ J.

For a given process at constant pressure, w is positive. This means that the process involves ________.

The value of ΔH° for the reaction below is -126 kJ. ________ kj are released when 2.00 mol of NaOH is formed in the reaction? 2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

The temperature of a 11.8 g sample of calcium carbonate [CaCO3 (s)] increases from 24.8 °C to 38.0 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed?

Given the following reactions N2 (g) + O2 (g) → 2NO (g)ΔH = +180.7 kJ 2NO( g) + O2 (g) → 2NO2 (g)ΔH = -113.1 kJ The enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO2 (g) → N2 (g) + 2O2 (g) Is ________ kJ.

For which one of the following reactions is the value of ΔH°rxn equal to ΔH°f for the product?

One joule equals 1 kg-m2/s2.

When work is done on a system, w will be a ________ value.

Which of the following is a statement of the first law of thermodynamics?

The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 2.12-kg block of copper from 25.0 °C to 99.9 °C?

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

Given the data in the table below, ΔH°rxn for the reaction 3NO2 (g) + H2O (l) → 2HNO3 (aq) + NO (g) Is ________ kJ.

Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2H3AsO4 → Ca(H2AsO4)2 + 2H2O Is ________ kJ.

The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is ________ kcal.

Calculate the work (kJ)done during a reaction in which the internal volume expands from 14 L to 50 L against a vacuum (an outside pressure of 0 atm).

The energy released by combustion of 1 g of a substance is called the ________ of the substance.

The standard enthalpy change of a reaction is the enthalpy change when all reactants and products are at ________ pressure and a specific temperature.

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The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH₄ (g) + 3Cl₂ (g) → CHCl₃ (l) + 3HCl (g)

In the reaction below, ΔH°_f is zero for ________. Ni (s) + 2CO (g) + 2PF₃ (g) → Ni(CO)₂(PF₃)₂ (l)

The value of ΔH° for the reaction below is -126 kJ. ________ kj are released when 2.00 mol of NaOH is formed in the reaction? 2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

The temperature of a 11.8 g sample of calcium carbonate [CaCO₃ (s)] increases from 24.8 °C to 38.0 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed?

Given the following reactions N₂ (g) + O₂ (g) → 2NO (g)ΔH = +180.7 kJ 2NO( g) + O₂ (g) → 2NO₂ (g)ΔH = -113.1 kJ The enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO₂ (g) → N₂ (g) + 2O₂ (g) Is ________ kJ.

For which one of the following reactions is the value of ΔH°_rxn equal to ΔH°_f for the product?

One joule equals 1 kg-m²/s².

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l)△H = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.80 g of methane is combusted at constant pressure.

Given the data in the table below, ΔH°_rxn for the reaction 3NO₂ (g) + H₂O (l) → 2HNO₃ (aq) + NO (g) Is ________ kJ.

Given the data in the table below, ΔH°_rxn for the reaction Ca(OH)₂ + 2H₃AsO₄ → Ca(H₂AsO₄)₂ + 2H₂O Is ________ kJ.