Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H2O2(l)→ 2 H2O(l)+ O2(g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure.

A) -26.5 kJ B) -13.3 kJ C) -0.0189 kJ D) 1.25 kJ E) -2.65 × 104 kJ A) -26.5 kJ B) -13.3 kJ C) -0.0189 kJ D) 1.25 kJ E) -2.65 × 104 kJ

According to the following thermochemical equation,what mass of H2O (in g)must form in order to produce 975 kJ of energy? SiO2(s)+ 4 HF(g)→ SiF4(g)+ 2 H2O(l)ΔH°rxn = -184 kJ

A) 68.0 g B) 102 g C) 54.1 g D) 191 g E) 95.5 g A) 68.0 g B) 102 g C) 54.1 g D) 191 g E) 95.5 g

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s)+ 3 O2(g)→ 2 SO3(g)ΔH°rxn = ? Given: SO2(g)→ S(s)+ O2(g)ΔH°rxn = +296.8 kJ 2 SO2(g)+ O2(g)→ 2 SO3(g)ΔH°rxn = -197.8 kJ

A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ A) -494.6 kJ B) -692.4 kJ C) -791.4 kJ D) 1583 kJ E) -293.0 kJ

According to the following reaction,how much energy is required to decompose 56.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s)→ 3 Fe(s)+ 2 O2(g)ΔH°rxn = +1118 kJ

A) 1.35 × 105 kJ B) 1.07 × 104 kJ C) 2.70 × 105 kJ D) 5.41 × 105 kJ E) 8.11 × 105 kJ A) 1.35 × 105 kJ B) 1.07 × 104 kJ C) 2.70 × 105 kJ D) 5.41 × 105 kJ E) 8.11 × 105 kJ

Exam 6: Thermochemistry

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂O₂(l)→ 2 H₂O(l)+ O₂(g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure.

(Multiple Choice)

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Question 121

Define heat capacity.

(Multiple Choice)

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Question 122

When 5.50 g of Ba(s)is added to 100.00 g of water in a container open to the atmosphere,the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 61.16°C.If the specific heat of the solution is 4.18 J/(g ∙ °C),calculate for the reaction,as written. Ba(s)+ 2 H₂O(l)→ Ba(OH)₂(aq)+ H₂(g) = ?

(Multiple Choice)

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Question 123

Choose the reaction that illustrates ΔH°_f for KHCO₃.

(Multiple Choice)

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Question 124

Define specific heat capacity.

(Multiple Choice)

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Question 125

The specific heat of copper is 0.385 J/(g ∙ °C).If 34.2 g of copper,initially at 25.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

(Multiple Choice)

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Question 126

According to the following thermochemical equation,what mass of H₂O (in g)must form in order to produce 975 kJ of energy? SiO₂(s)+ 4 HF(g)→ SiF₄(g)+ 2 H₂O(l)ΔH°_rxn= -184 kJ

(Multiple Choice)

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Question 127

Calculate the change in internal energy (ΔE)for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 16.0 L in volume at 2.00 atm.(Remember that 101.3 J = 1 L^∙atm)

(Multiple Choice)

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Question 128

Energy that is associated with the position or composition of an object is called

(Multiple Choice)

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Question 129

A balloon is inflated from 0.0100 L to 0.600 L against an external pressure of 10.00 atm.How much work is done in joules? 101.3 J = 1 L × atm

(Multiple Choice)

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Question 130

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 9.20°C? (The specific heat of the solution is 3.74 J/g ∙ K.)

(Multiple Choice)

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Question 131

Two solutions,initially at 24.60°C,are mixed in a coffee cup calorimeter.When a 100.0 mL volume of 0.100 M AgNO₃ solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution,the temperature in the calorimeter rises to 25.30°C.Determine the DH°_rxn for the reaction as written below.Assume that the density and heat capacity of the solutions is the same as that of water. NaCl(aq)+ AgNO₃(aq)→ AgCl(s)+ NaNO₃(aq)DH°_rxn = ?

(Multiple Choice)

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Question 132

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction: 2 S(s)+ 3 O₂(g)→ 2 SO₃(g)ΔH°_rxn= ? Given: SO₂(g)→ S(s)+ O₂(g)ΔH°_rxn= +296.8 kJ 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)ΔH°_rxn= -197.8 kJ

(Multiple Choice)

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Question 133

Choose the thermochemical equation that illustrates ΔH°_f for Li₂SO₄.

(Multiple Choice)

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Question 134

Which of the following statements is TRUE?

(Multiple Choice)

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Question 135

Calculate the change internal energy (ΔE)for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings.

(Multiple Choice)

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Question 136

A 6.55 g sample of aniline (C₆H₅NH₂,molar mass = 93.13 g/mol)was combusted in a bomb calorimeter.If the temperature rose by 32.9°C,use the information below to determine the heat capacity of the calorimeter. 4 C₆H₅NH₂(l)+ 35 O₂(g)→ 24 CO₂(g)+ 14 H₂O(g)+ 4 NO₂(g) ΔH°_rxn= -1.28 × 10⁴ kJ

(Multiple Choice)

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Question 137

The law of ________ states that energy that can be neither created nor destroyed.

(Multiple Choice)

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Question 138

According to the following reaction,how much energy is required to decompose 56.0 kg of Fe₃O₄? The molar mass of Fe₃O₄is 231.55 g/mol. Fe₃O₄(s)→ 3 Fe(s)+ 2 O₂(g)ΔH°_rxn= +1118 kJ

(Multiple Choice)

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Question 139

When 50.0 mL of 0.400 M Ca(NO₃)₂ is added to 50.0 mL of 0.800 M NaF,CaF₂ precipitates,as shown in the net ionic equation below.The initial temperature of both solutions is 22.0°C.Assuming that the reaction goes to completion,and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C),calculate the final temperature of the solution. Ca²⁺(aq)+ 2 F^-(aq)→ CaF₂(s)ΔH° = -11.5 kJ

(Multiple Choice)

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Question 140

Showing 121 - 140 of 143

Exam 6: Thermochemistry

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H2O2(l)→ 2 H2O(l)+ O2(g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure.

Define heat capacity.

Choose the reaction that illustrates ΔH°f for KHCO3.

Define specific heat capacity.

The specific heat of copper is 0.385 J/(g ∙ °C).If 34.2 g of copper,initially at 25.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

According to the following thermochemical equation,what mass of H2O (in g)must form in order to produce 975 kJ of energy? SiO2(s)+ 4 HF(g)→ SiF4(g)+ 2 H2O(l)ΔH°rxn = -184 kJ

Calculate the change in internal energy (ΔE)for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 16.0 L in volume at 2.00 atm.(Remember that 101.3 J = 1 L∙atm)

Energy that is associated with the position or composition of an object is called

A balloon is inflated from 0.0100 L to 0.600 L against an external pressure of 10.00 atm.How much work is done in joules? 101.3 J = 1 L × atm

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 9.20°C? (The specific heat of the solution is 3.74 J/g ∙ K.)

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 S(s)+ 3 O2(g)→ 2 SO3(g)ΔH°rxn = ? Given: SO2(g)→ S(s)+ O2(g)ΔH°rxn = +296.8 kJ 2 SO2(g)+ O2(g)→ 2 SO3(g)ΔH°rxn = -197.8 kJ

Choose the thermochemical equation that illustrates ΔH°f for Li2SO4.

Which of the following statements is TRUE?

Calculate the change internal energy (ΔE)for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings.

A 6.55 g sample of aniline (C6H5NH2,molar mass = 93.13 g/mol)was combusted in a bomb calorimeter.If the temperature rose by 32.9°C,use the information below to determine the heat capacity of the calorimeter. 4 C6H5NH2(l)+ 35 O2(g)→ 24 CO2(g)+ 14 H2O(g)+ 4 NO2(g) ΔH°rxn = -1.28 × 104 kJ

The law of ________ states that energy that can be neither created nor destroyed.

According to the following reaction,how much energy is required to decompose 56.0 kg of Fe3O4? The molar mass of Fe3O4 is 231.55 g/mol. Fe3O4(s)→ 3 Fe(s)+ 2 O2(g)ΔH°rxn = +1118 kJ

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Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂O₂(l)→ 2 H₂O(l)+ O₂(g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure.

Choose the reaction that illustrates ΔH°_f for KHCO₃.

According to the following thermochemical equation,what mass of H₂O (in g)must form in order to produce 975 kJ of energy? SiO₂(s)+ 4 HF(g)→ SiF₄(g)+ 2 H₂O(l)ΔH°_rxn= -184 kJ

Calculate the change in internal energy (ΔE)for a system that is absorbing 35.8 kJ of heat and is expanding from 8.00 to 16.0 L in volume at 2.00 atm.(Remember that 101.3 J = 1 L^∙atm)

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction: 2 S(s)+ 3 O₂(g)→ 2 SO₃(g)ΔH°_rxn= ? Given: SO₂(g)→ S(s)+ O₂(g)ΔH°_rxn= +296.8 kJ 2 SO₂(g)+ O₂(g)→ 2 SO₃(g)ΔH°_rxn= -197.8 kJ

Choose the thermochemical equation that illustrates ΔH°_f for Li₂SO₄.

According to the following reaction,how much energy is required to decompose 56.0 kg of Fe₃O₄? The molar mass of Fe₃O₄is 231.55 g/mol. Fe₃O₄(s)→ 3 Fe(s)+ 2 O₂(g)ΔH°_rxn= +1118 kJ