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 1.70 g of methane is combusted at constant pressure.

A) -94.6 B) 0.0306 C) -0.0106 D) 32.7 E) -9.46 × 104 A) -94.6 B) 0.0306 C) -0.0106 D) 32.7 E) -9.46 × 104

The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.

A) 88.0 B) 1.13 C) 4.89 D) 6.88 × E) -88.0 A) 88.0 B) 1.13 C) 4.89 D) 6.88 × E) -88.0

Exam 5: Thermochemistry

What is the enthalpy change (in kJ)of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.)

(Multiple Choice)

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Question 121

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 122

The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.

(Multiple Choice)

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Question 123

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

(Multiple Choice)

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Question 124

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 1.70 g of methane is combusted at constant pressure.

(Multiple Choice)

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(71)

Question 125

Renewable energy sources are essentially inexhaustible.

(True/False)

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Question 126

The molar heat capacity of a compound with the formula C₂H₆SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.

(Multiple Choice)

4.8/5

(76)

Question 127

A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 20.2 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is __________ kJ.

(Multiple Choice)

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(88)

Question 128

The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.

(Multiple Choice)

4.8/5

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Question 129

One joule equals 1 kg ∙ m²/s².

(True/False)

4.7/5

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Question 130

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 4.0 mol of HBr is formed in this reaction. H₂ (g)+ Br₂ (g)→ 2HBr (g)

(Multiple Choice)

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Question 131

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction. H₂ (g)+ Br₂ (g)→ 2HBr (g)

(Multiple Choice)

4.9/5

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Question 132

The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 10.1-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)

5.0/5

(90)

Question 133

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

(Multiple Choice)

4.8/5

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Question 134

A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W)= 1 J/sec]

(Multiple Choice)

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Question 135

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 136

Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100°C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

(Short Answer)

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(76)

Question 137

For which one of the following reactions is ΔH°_rxn equal to the heat of formation of the product?

(Multiple Choice)

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Question 138

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)

4.8/5

(76)

Question 139

A sample of calcium carbonate [CaCO₃ (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °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)

4.9/5

(74)

Question 140

Showing 121 - 140 of 148

Exam 5: Thermochemistry

What is the enthalpy change (in kJ)of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.)

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

The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.

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

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 1.70 g of methane is combusted at constant pressure.

Renewable energy sources are essentially inexhaustible.

The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.

A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 20.2 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is __________ kJ.

The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.

One joule equals 1 kg ∙ m2/s2.

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 4.0 mol of HBr is formed in this reaction. H2 (g)+ Br2 (g)→ 2HBr (g)

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction. H2 (g)+ Br2 (g)→ 2HBr (g)

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

A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W)= 1 J/sec]

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

Given the equation H2O (l)→ H2O (g)ΔHrxn = 40.7 kJ at 100°C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product?

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.

A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams)of the sample?

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Additional Aspects of Aqueous Equilibria

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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 1.70 g of methane is combusted at constant pressure.

The molar heat capacity of a compound with the formula C₂H₆SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.

One joule equals 1 kg ∙ m²/s².

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 4.0 mol of HBr is formed in this reaction. H₂ (g)+ Br₂ (g)→ 2HBr (g)

The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction. H₂ (g)+ Br₂ (g)→ 2HBr (g)

Given the equation H₂O (l)→ H₂O (g)ΔH_rxn= 40.7 kJ at 100°C Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

For which one of the following reactions is ΔH°_rxn equal to the heat of formation of the product?

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.

A sample of calcium carbonate [CaCO₃ (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams)of the sample?