Given the data in the table below, ΔH°rxn for the reaction IF5 (g) + F2 (g) → IF7 (g) Is ________ kJ.

A) 1801 B) -1801 C) 121 D) -121 E) -101 A) 1801 B) -1801 C) 121 D) -121 E) -101

For the species in the reaction below, ΔH°f is zero for ________. 2Co (s) + H2 (g) + 8PF3 (g) → 2HCo(PF3)4 (l)

A) Co (s) B) H2 (g) C) PF3 (g) D) HCo(PF3)4 (l) E) both Co(s)and H2 (g) A) Co (s) B) H2 (g) C) PF3 (g) D) HCo(PF3)4 (l) E) both Co(s)and H2 (g)

Given the following reactions Fe2O3 (s) + 3CO (s) → 2Fe (s)+ 3CO2 (g)ΔH = -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe2O3 with CO 3Fe2O3 (s) + CO (g) → CO2 (g) + 2 Fe3O4 (s) Is ________ kJ.

A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109 A) -59.0 B) 40.5 C) -15.5 D) -109 E) +109

The value of ΔH° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) → 2HCl (g) The value of ΔH°f for HCl (g)is ________ kJ/mol.

A) -3.72 × 102 B) -1.27 × 102 C) -93.0 D) -186 E) +186 A) -3.72 × 102 B) -1.27 × 102 C) -93.0 D) -186 E) +186

The reaction 4Al (s) + 3O2 (g) → 2Al2O3 (s) ΔH° = -3351 kJ Is ________, and therefore heat is ________ by the reaction.

A) endothermic, released B) endothermic, absorbed C) exothermic, released D) exothermic, absorbed E) thermoneutral, neither released nor absorbed A) endothermic, released B) endothermic, absorbed C) exothermic, released D) exothermic, absorbed E) thermoneutral, neither released nor absorbed

Exam 5: Thermochemistry

Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100 °C Calculate the mass of liquid water (in grams)at 100 °C that can converted to vapor by absorbing 2400 J of heat.

(Short Answer)

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Question 101

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

(Multiple Choice)

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Question 102

Given the data in the table below, ΔH°_rxn for the reaction IF₅ (g) + F₂ (g) → IF₇ (g) Is ________ kJ.

(Multiple Choice)

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Question 103

For the species in the reaction below, ΔH°_f is zero for ________. 2Co (s) + H₂ (g) + 8PF₃ (g) → 2HCo(PF₃)₄ (l)

(Multiple Choice)

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Question 104

A sample of iron absorbs 81.0 J of heat, upon which the temperature of the sample increases from 19.7 °C to 28.2 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams)of the sample?

(Multiple Choice)

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Question 105

Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. (1 mile = 1.6093 km, 1lb = 453.59 g).

(Multiple Choice)

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Question 106

Given the following reactions Fe₂O₃ (s) + 3CO (s) → 2Fe (s)+ 3CO₂ (g)ΔH = -28.0 kJ 3Fe (s) + 4CO₂ (s) → 4CO (g) + Fe₃O₄ (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe₂O₃ with CO 3Fe₂O₃ (s) + CO (g) → CO₂ (g) + 2 Fe₃O₄ (s) Is ________ kJ.

(Multiple Choice)

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Question 107

The units of specific heat are ________.

(Multiple Choice)

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Question 108

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

(Multiple Choice)

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Question 109

A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ________ g.

(Multiple Choice)

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Question 110

Of the following, which one is a state function?

(Multiple Choice)

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Question 111

The value of ΔH° for the reaction below is -186 kJ. H₂ (g) + Cl₂ (g) → 2HCl (g) The value of ΔH°_f for HCl (g)is ________ kJ/mol.

(Multiple Choice)

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Question 112

The reaction 4Al (s) + 3O₂ (g) → 2Al₂O₃(s) ΔH° = -3351 kJ Is , and therefore heat is by the reaction.

(Multiple Choice)

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Question 113

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

(Multiple Choice)

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Question 114

A 5.00-g sample of copper metal at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is 0.38 J/g-K.

(Multiple Choice)

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Question 115

The kinetic energy of a 26.9-g object moving at a speed of 81.9 m/s is ________ J.

(Multiple Choice)

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Question 116

The most abundant fossil fuel is ________.

(Multiple Choice)

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Question 117

Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg)traveling at 12.0 mile/hr (5.36 m/s).

(Multiple Choice)

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Question 118

The value of ΔH° for the reaction below is -72 kJ. ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction. H₂ (g) + Br₂ (g) → 2HBr (g)

(Multiple Choice)

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Question 119

When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is ________ J. (The specific heat of water is 4.18 J/g-°C.)

(Short Answer)

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Question 120

Showing 101 - 120 of 154

Exam 5: Thermochemistry

Given the equation H2O (l)→ H2O (g)ΔHrxn = 40.7 kJ at 100 °C Calculate the mass of liquid water (in grams)at 100 °C that can converted to vapor by absorbing 2400 J of heat.

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

Given the data in the table below, ΔH°rxn for the reaction IF5 (g) + F2 (g) → IF7 (g) Is ________ kJ.

For the species in the reaction below, ΔH°f is zero for ________. 2Co (s) + H2 (g) + 8PF3 (g) → 2HCo(PF3)4 (l)

A sample of iron absorbs 81.0 J of heat, upon which the temperature of the sample increases from 19.7 °C to 28.2 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams)of the sample?

Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. (1 mile = 1.6093 km, 1lb = 453.59 g).

Given the following reactions Fe2O3 (s) + 3CO (s) → 2Fe (s)+ 3CO2 (g)ΔH = -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe3O4 (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe2O3 with CO 3Fe2O3 (s) + CO (g) → CO2 (g) + 2 Fe3O4 (s) Is ________ kJ.

The units of specific heat are ________.

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

A sample of aluminum metal absorbs 11.2 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ________ g.

Of the following, which one is a state function?

The value of ΔH° for the reaction below is -186 kJ. H2 (g) + Cl2 (g) → 2HCl (g) The value of ΔH°f for HCl (g)is ________ kJ/mol.

The reaction 4Al (s) + 3O2 (g) → 2Al2O3 (s) ΔH° = -3351 kJ Is ________, and therefore heat is ________ by the reaction.

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

A 5.00-g sample of copper metal at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is 0.38 J/g-K.

The kinetic energy of a 26.9-g object moving at a speed of 81.9 m/s is ________ J.

The most abundant fossil fuel is ________.

Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg)traveling at 12.0 mile/hr (5.36 m/s).

The value of ΔH° for the reaction below is -72 kJ. ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction. H2 (g) + Br2 (g) → 2HBr (g)

When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is ________ J. (The specific heat of water is 4.18 J/g-°C.)

Introduction: Matter and Measurement

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Additional Aspects of Aqueous Equilibria

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Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100 °C Calculate the mass of liquid water (in grams)at 100 °C that can converted to vapor by absorbing 2400 J of heat.

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

Given the data in the table below, ΔH°_rxn for the reaction IF₅ (g) + F₂ (g) → IF₇ (g) Is ________ kJ.

For the species in the reaction below, ΔH°_f is zero for ________. 2Co (s) + H₂ (g) + 8PF₃ (g) → 2HCo(PF₃)₄ (l)

Given the following reactions Fe₂O₃ (s) + 3CO (s) → 2Fe (s)+ 3CO₂ (g)ΔH = -28.0 kJ 3Fe (s) + 4CO₂ (s) → 4CO (g) + Fe₃O₄ (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe₂O₃ with CO 3Fe₂O₃ (s) + CO (g) → CO₂ (g) + 2 Fe₃O₄ (s) Is ________ kJ.

The value of ΔH° for the reaction below is -186 kJ. H₂ (g) + Cl₂ (g) → 2HCl (g) The value of ΔH°_f for HCl (g)is ________ kJ/mol.

The reaction 4Al (s) + 3O₂ (g) → 2Al₂O₃(s) ΔH° = -3351 kJ Is , and therefore heat is by the reaction.

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

The value of ΔH° for the reaction below is -72 kJ. ________ kJ of heat are released when 5.5 mol of HBr is formed in this reaction. H₂ (g) + Br₂ (g) → 2HBr (g)