Use the information provided to determine H° for the following reaction: H° (kJ ) 3Fe2O3(s) + CO(g) → 2Fe3O4(s) + CO2(g) H° = ? Fe2O3(s) -824 Fe3O4(s) -1118 CO(g) -111 CO2(g) -394

A) +277 kJ mol-1 B) -577 kJ mol-1 C) -47 kJ mol-1 D) +144 kJ mol-1 E) -111 kJ mol-1 A) +277 kJ mol-1 B) -577 kJ mol-1 C) -47 kJ mol-1 D) +144 kJ mol-1 E) -111 kJ mol-1 C

How much heat is absorbed when 50.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5C(s) + 2SO2(g) → CS2(l) + 4CO(g) H° = 239.9 kJ

A) 199.7 kJ B) 239.9 kJ C) 998.3 kJ D) 2398 kJ A) 199.7 kJ B) 239.9 kJ C) 998.3 kJ D) 2398 kJ

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

A) -494.6 kJ mol-1 B) -692.4 kJ mol-1 C) -791.4 kJ mol-1 D) 1583 kJ mol-1 E) -293.0 kJ mol-1 A) -494.6 kJ mol-1 B) -692.4 kJ mol-1 C) -791.4 kJ mol-1 D) 1583 kJ mol-1 E) -293.0 kJ mol-1

Use the information provided to determine H° for the following reaction: H°(kJ ) CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) H° = ? CH4(g) -75 CCl4(g) -96 HCl(g) -92

A) -389 kJ mol-1 B) -113 kJ mol-1 C) +113 kJ mol-1 D) -71 kJ mol-1 E) +79 kJ mol-1 A) -389 kJ mol-1 B) -113 kJ mol-1 C) +113 kJ mol-1 D) -71 kJ mol-1 E) +79 kJ mol-1

Exam 6: Thermochemistry

Use the information provided to determine H° for the following reaction: H° (kJ ) 3Fe₂O₃(s) + CO(g) → 2Fe₃O₄(s) + CO₂(g) H°= ? Fe₂O₃(s) -824 Fe₃O₄(s) -1118 CO(g) -111 CO₂(g) -394

Free

(Multiple Choice)

4.8/5

(28)

Question 1

Correct Answer:

Verified

Given w = 0, an endothermic reaction has which of the following properties?

Free

(Multiple Choice)

4.8/5

(35)

Question 2

Correct Answer:

Verified

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s) H°= -852 kJ

Free

(Multiple Choice)

4.8/5

(23)

Question 3

Correct Answer:

Verified

An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

(Multiple Choice)

4.9/5

(28)

Question 4

Identify an energy source that is non-renewable.

(Multiple Choice)

4.8/5

(41)

Question 5

How much heat is absorbed when 50.00 g of C(s) reacts in the presence of excess SO₂(g) to produce CS₂(l) and CO(g) according to the following chemical equation? 5C(s) + 2SO₂(g) → CS₂(l) + 4CO(g) H° = 239.9 kJ

(Multiple Choice)

4.7/5

(31)

Question 6

Calculate the final temperature of a 38.1 g piece of graphitic carbon, originally at 100.0 °C, placed inside a coffee cup calorimeter containing 68.0 mL of water at 24.6 °C. The specific heat capacity of water is 4.184 J g^-1 °C^-1, the specific heat capacity of graphitic carbon is 0.709 J g^-1 °C^-1, and the density of water is 1.00 g mL^-1.

(Multiple Choice)

4.8/5

(41)

Question 7

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J g^-1°C^-1.

(Multiple Choice)

4.8/5

(32)

Question 8

Which of the following processes is endothermic?

(Multiple Choice)

4.9/5

(31)

Question 9

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

(Multiple Choice)

4.7/5

(35)

Question 10

According to the following thermochemical equation, what mass of HF (in g) must react to produce 345 kJ of energy? Assume excess SiO₂. SiO₂(s) + 4HF(g) → SiF₄(g) + 2H₂O(l) H°= -184 kJ

(Multiple Choice)

4.8/5

(30)

Question 11

Calculate the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 bar. (Remember that 100 J = 1 L bar)

(Multiple Choice)

4.8/5

(35)

Question 12

Match the following. --ΔU

(Multiple Choice)

4.9/5

(36)

Question 13

Match the following. -energy associated with the motion of an object

(Multiple Choice)

4.8/5

(38)

Question 14

Match the following. --w

(Multiple Choice)

4.8/5

(39)

Question 15

Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.0 15 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00 °C to 31.45 °C. If the specific heat of the solution is 4.18 J , calculate ΔH for the reaction, as written. 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g) H= ?

(Multiple Choice)

4.7/5

(38)

Question 16

A piece of uranium with a mass of 12.1 g and an initial temperature of 60.2 °C was placed inside a coffee cup calorimeter. The temperature of the water inside the calorimeter increased from 22.8 °C to 23.9 °C. The specific heat capacity of water is 4.184 J g^-1 °C^-1 and the specific heat capacity of uranium is 0.116 J g^-1 °C^-1. Calculate the mass of water contained inside the calorimeter.

(Multiple Choice)

4.9/5

(33)

Question 17

The specific heat capacity of liquid water is 4.184 J . How many joules of heat are needed to raise the temperature of 7.00 g of water from 33.0 °C to 76.0 °C?

(Multiple Choice)

4.7/5

(32)

Question 18

A balloon is inflated from 0.0100 L to 0.500 L against an external pressure of 10.00 bar. How much work is done in joules? (100 J = 1 L bar)

(Multiple Choice)

4.9/5

(36)

Question 19

Use the information provided to determine H° for the following reaction: H°(kJ ) CH₄(g) + 4 Cl₂(g) → CCl₄(g) + 4 HCl(g) H°= ? CH₄(g) -75 CCl₄(g) -96 HCl(g) -92

(Multiple Choice)

4.7/5

(29)

Question 20

Showing 1 - 20 of 161

Exam 6: Thermochemistry

Use the information provided to determine H° for the following reaction: H° (kJ ) 3Fe2O3(s) + CO(g) → 2Fe3O4(s) + CO2(g) H° = ? Fe2O3(s) -824 Fe3O4(s) -1118 CO(g) -111 CO2(g) -394

Given w = 0, an endothermic reaction has which of the following properties?

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s) H° = -852 kJ

An unknown metal alloy, mass = 26.3 g, has a temperature increase of 8.31 °C after a heat transfer of 94.0 J. Calculate the specific heat capacity of the alloy.

Identify an energy source that is non-renewable.

How much heat is absorbed when 50.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation? 5C(s) + 2SO2(g) → CS2(l) + 4CO(g) H° = 239.9 kJ

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J g-1 °C-1.

Which of the following processes is endothermic?

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

According to the following thermochemical equation, what mass of HF (in g) must react to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(l) H° = -184 kJ

Calculate the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 6.00 L in volume at 1.50 bar. (Remember that 100 J = 1 L bar)

Match the following. --ΔU

Match the following. -energy associated with the motion of an object

Match the following. --w

The specific heat capacity of liquid water is 4.184 J . How many joules of heat are needed to raise the temperature of 7.00 g of water from 33.0 °C to 76.0 °C?

A balloon is inflated from 0.0100 L to 0.500 L against an external pressure of 10.00 bar. How much work is done in joules? (100 J = 1 L bar)

Use the information provided to determine H° for the following reaction: H°(kJ ) CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) H° = ? CH4(g) -75 CCl4(g) -96 HCl(g) -92

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Use the information provided to determine H° for the following reaction: H° (kJ ) 3Fe₂O₃(s) + CO(g) → 2Fe₃O₄(s) + CO₂(g) H°= ? Fe₂O₃(s) -824 Fe₃O₄(s) -1118 CO(g) -111 CO₂(g) -394

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s) H°= -852 kJ

How much heat is absorbed when 50.00 g of C(s) reacts in the presence of excess SO₂(g) to produce CS₂(l) and CO(g) according to the following chemical equation? 5C(s) + 2SO₂(g) → CS₂(l) + 4CO(g) H° = 239.9 kJ

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J g^-1°C^-1.

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

According to the following thermochemical equation, what mass of HF (in g) must react to produce 345 kJ of energy? Assume excess SiO₂. SiO₂(s) + 4HF(g) → SiF₄(g) + 2H₂O(l) H°= -184 kJ

Use the information provided to determine H° for the following reaction: H°(kJ ) CH₄(g) + 4 Cl₂(g) → CCl₄(g) + 4 HCl(g) H°= ? CH₄(g) -75 CCl₄(g) -96 HCl(g) -92