The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + 2H2 (g) How many kJ of heat are consumed when 15.5 g of CH3OH (l)decomposes as shown in the equation?

A) 0.48 kJ B) 62.0 kJ C) 1.3 × 102 kJ D) 32 kJ E) 8.3 kJ A) 0.48 kJ B) 62.0 kJ C) 1.3 × 102 kJ D) 32 kJ E) 8.3 kJ

The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) → 2H2O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H2 (g) + 2O2 (g) → 4H2O (g)

A) -483.6 B) -967.2 C) 2.34 × 105 D) 483.6 E) 967.2 A) -483.6 B) -967.2 C) 2.34 × 105 D) 483.6 E) 967.2

Given the following reactions N2 (g) + 2O2 (g) → 2NO2 (g)ΔH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (g) + O2 (g) → 2NO (g) Is ________ kJ.

A) 180.6 B) -47.8 C) 47.8 D) 90.3 E) -180.6 A) 180.6 B) -47.8 C) 47.8 D) 90.3 E) -180.6

The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + 2H2 (g) How many kJ of heat are consumed when 5.10 g of H2 (g)is formed as shown in the equation?

A) 162 kJ B) 62.0 kJ C) 128 kJ D) 653 kJ E) 326 kJ A) 162 kJ B) 62.0 kJ C) 128 kJ D) 653 kJ E) 326 kJ

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2 (l) → 2H2O (l)+ O2 (g)△H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.50 g of hydrogen peroxide decomposes at constant pressure?

A) -8.65 kJ B) -4.32 kJ C) -0.0578 kJ D) 3.84 kJ E) -8.65 × 103 kJ A) -8.65 kJ B) -4.32 kJ C) -0.0578 kJ D) 3.84 kJ E) -8.65 × 103 kJ

Given the following reactions CaCO3 (s) → CaO (s) + CO2 (g)ΔH = 178.1 kJ C (s, graphite) + O2 (g) → CO2 (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO3 (s) → CaO (s) + C (s, graphite) + O2 (g) Is ________ kJ.

A) 215.4 B) 571.6 C) -215.4 D) -571.6 E) 7.01 × 104 A) 215.4 B) 571.6 C) -215.4 D) -571.6 E) 7.01 × 104

Exam 5: Thermochemistry

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 38.5 g of O₂ (g)reacts with excess CO. 2CO (g) + O₂ (g) → 2CO₂ (g)

(Multiple Choice)

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Question 121

Units of energy include newtons, joules, and calories.

(True/False)

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Question 122

The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l) → CO (g) + 2H₂ (g) How many kJ of heat are consumed when 15.5 g of CH₃OH (l)decomposes as shown in the equation?

(Multiple Choice)

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Question 123

The enthalpy change for the following reaction is -483.6 kJ: 2H₂ (g) + O₂ (g) → 2H₂O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H₂ (g) + 2O₂ (g) → 4H₂O (g)

(Multiple Choice)

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Question 124

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

(Multiple Choice)

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Question 125

At what velocity (m/s)must a 417.3 g object be moving in order to possess a kinetic energy of 3.2 J?

(Multiple Choice)

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Question 126

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J)is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

(Multiple Choice)

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Question 127

A sample of calcium carbonate [CaCO₃ (s)] absorbs 40.3 J of heat, upon which the temperature of the sample increases from 20.8 °C to 27.3 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams)of the sample?

(Multiple Choice)

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Question 128

Given the following reactions N₂ (g) + 2O₂ (g) → 2NO₂ (g)ΔH = 66.4 kJ 2NO (g) + O₂ (g) → 2NO₂ (g) ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N₂ (g) + O₂ (g) → 2NO (g) Is ________ kJ.

(Multiple Choice)

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Question 129

The units of heat capacity are ________.

(Multiple Choice)

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Question 130

The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l) → CO (g) + 2H₂ (g) How many kJ of heat are consumed when 5.10 g of H₂ (g)is formed as shown in the equation?

(Multiple Choice)

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Question 131

When a system ________, ΔE is always negative.

(Multiple Choice)

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Question 132

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H₂O₂ (l) → 2H₂O (l)+ O₂ (g)△H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.50 g of hydrogen peroxide decomposes at constant pressure?

(Multiple Choice)

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Question 133

The value of ΔE for a system that performs 139 kJ of work on its surroundings and gains 54kJ of heat is ________ kJ.

(Multiple Choice)

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Question 134

Given the following reactions CaCO₃ (s) → CaO (s) + CO₂ (g)ΔH = 178.1 kJ C (s, graphite) + O₂ (g) → CO₂ (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO₃ (s) → CaO (s) + C (s, graphite) + O₂ (g) Is ________ kJ.

(Multiple Choice)

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Question 135

Of the substances below, the highest fuel value is obtained from ________.

(Multiple Choice)

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Question 136

ΔH for an endothermic process is while ΔH for an exothermic process is .

(Multiple Choice)

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Question 137

Of the following, ΔH°_f is not zero for ________.

(Multiple Choice)

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Question 138

The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na₂O₂ with water is ________ kJ. 2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

(Multiple Choice)

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Question 139

A ΔH corresponds to an process.

(Multiple Choice)

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Question 140

Showing 121 - 140 of 154

Exam 5: Thermochemistry

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 38.5 g of O2 (g)reacts with excess CO. 2CO (g) + O2 (g) → 2CO2 (g)

Units of energy include newtons, joules, and calories.

The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + 2H2 (g) How many kJ of heat are consumed when 15.5 g of CH3OH (l)decomposes as shown in the equation?

The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) → 2H2O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H2 (g) + 2O2 (g) → 4H2O (g)

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

At what velocity (m/s)must a 417.3 g object be moving in order to possess a kinetic energy of 3.2 J?

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J)is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

A sample of calcium carbonate [CaCO3 (s)] absorbs 40.3 J of heat, upon which the temperature of the sample increases from 20.8 °C to 27.3 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams)of the sample?

Given the following reactions N2 (g) + 2O2 (g) → 2NO2 (g)ΔH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (g) + O2 (g) → 2NO (g) Is ________ kJ.

The units of heat capacity are ________.

The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + 2H2 (g) How many kJ of heat are consumed when 5.10 g of H2 (g)is formed as shown in the equation?

When a system ________, ΔE is always negative.

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2 (l) → 2H2O (l)+ O2 (g)△H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.50 g of hydrogen peroxide decomposes at constant pressure?

The value of ΔE for a system that performs 139 kJ of work on its surroundings and gains 54kJ of heat is ________ kJ.

Given the following reactions CaCO3 (s) → CaO (s) + CO2 (g)ΔH = 178.1 kJ C (s, graphite) + O2 (g) → CO2 (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO3 (s) → CaO (s) + C (s, graphite) + O2 (g) Is ________ kJ.

Of the substances below, the highest fuel value is obtained from ________.

ΔH for an endothermic process is ________ while ΔH for an exothermic process is ________.

Of the following, ΔH°f is not zero for ________.

The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na2O2 with water is ________ kJ. 2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

A ________ ΔH corresponds to an ________ process.

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The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 38.5 g of O₂ (g)reacts with excess CO. 2CO (g) + O₂ (g) → 2CO₂ (g)

The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l) → CO (g) + 2H₂ (g) How many kJ of heat are consumed when 15.5 g of CH₃OH (l)decomposes as shown in the equation?

The enthalpy change for the following reaction is -483.6 kJ: 2H₂ (g) + O₂ (g) → 2H₂O (g) Therefore, the enthalpy change for the following reaction is ________ kJ. 4H₂ (g) + 2O₂ (g) → 4H₂O (g)

A sample of calcium carbonate [CaCO₃ (s)] absorbs 40.3 J of heat, upon which the temperature of the sample increases from 20.8 °C to 27.3 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams)of the sample?

Given the following reactions N₂ (g) + 2O₂ (g) → 2NO₂ (g)ΔH = 66.4 kJ 2NO (g) + O₂ (g) → 2NO₂ (g) ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N₂ (g) + O₂ (g) → 2NO (g) Is ________ kJ.

The value of ΔH° for the reaction below is +128.1 kJ: CH₃OH (l) → CO (g) + 2H₂ (g) How many kJ of heat are consumed when 5.10 g of H₂ (g)is formed as shown in the equation?

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H₂O₂ (l) → 2H₂O (l)+ O₂ (g)△H = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.50 g of hydrogen peroxide decomposes at constant pressure?

Given the following reactions CaCO₃ (s) → CaO (s) + CO₂ (g)ΔH = 178.1 kJ C (s, graphite) + O₂ (g) → CO₂ (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO₃ (s) → CaO (s) + C (s, graphite) + O₂ (g) Is ________ kJ.

ΔH for an endothermic process is while ΔH for an exothermic process is .

Of the following, ΔH°_f is not zero for ________.

The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 10.0 g of Na₂O₂ with water is ________ kJ. 2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

A ΔH corresponds to an process.