What is the overall chemical equation that results from the sum of the given steps? 2 C(s)+ 2 H2O(g)→ 2 CO(g)+ 2 H2(g) CO(g)+ H2O(g)→ CO2(g)+ H2(g) CO(g)+ 3 H2(g)→ CH4(g)+ H2O(g)

A) 2 C(s)+ 2 H2O(g)→ CO2(g)+ CH4(g) B) 2 C(s)+ 3 H2O(g)→ CO(g)+ CO2(g)+ 3 H2(g) C) 2 C(s)+ H2O(g)+ H2(g)→ CO(g)+ CH4(g) D) 2 CO(g)+ 2 H2(g)→ CH4(g)+ CO2(g) E) 2 C(s)+ CH4(g)+ 3 H2O(g)→ 3 CO(g)+ 5 H2(g) A) 2 C(s)+ 2 H2O(g)→ CO2(g)+ CH4(g) B) 2 C(s)+ 3 H2O(g)→ CO(g)+ CO2(g)+ 3 H2(g) C) 2 C(s)+ H2O(g)+ H2(g)→ CO(g)+ CH4(g) D) 2 CO(g)+ 2 H2(g)→ CH4(g)+ CO2(g) E) 2 C(s)+ CH4(g)+ 3 H2O(g)→ 3 CO(g)+ 5 H2(g)

When 1 mole of Fe2O3(s)reacts with H2(g)to form Fe(s)and H2O(g)by the following reaction,98.8 kJ of energy is absorbed. Fe2O3(s)+ 3 H2(g)→ 2 Fe(s)+ 3 H2O(g) (A) (B) Is the reaction endothermic or exothermic,and which of the enthalpy diagrams above Represents this reaction?

A) Endothermic; A B) Endothermic; B C) Exothermic; A D) Exothermic; B E) None of these A) Endothermic; A B) Endothermic; B C) Exothermic; A D) Exothermic; B E) None of these

Determine the enthalpy change for the decomposition of calcium carbonate CaCO3(s)→ CaO(s)+ CO2(g) Given the thermochemical equations below. Ca(OH)2(s)→ CaO(s)+ H2O( ) ΔrH° = 65.2 kJ/mol-rxn Ca(OH)2(s)+ CO2(g)→ CaCO3(s)+ H2O( ) ΔrH° = −113.8 kJ/mol-rxn C(s)+ O2(g)→ CO2(g) ΔrH° = −393.5 kJ/mol-rxn 2 Ca(s)+ O2(g)→ 2 CaO(s) ΔrH° = −1270.2 kJ/mol-rxn

A) +48.6 kJ/mol-rxn B) +179.0 kJ/mol-rxn C) +345.5 kJ/mol-rxn D) +441.0 kJ/mol-rxn E) +1711.7 kJ/mol-rxn A) +48.6 kJ/mol-rxn B) +179.0 kJ/mol-rxn C) +345.5 kJ/mol-rxn D) +441.0 kJ/mol-rxn E) +1711.7 kJ/mol-rxn

Commercial cold packs consist of solid ammonium nitrate and water.NH4NO3 absorbs 25.69 kJ of heat per mole dissolved in water.In a coffee-cup calorimeter,5.60 g NH4NO3 is dissolved in 100.0 g of water at 22.0 °C.What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/g⋅K.

A) 0.0 °C B) 17.9 °C C) 11.6 °C D) -54.8 °C E) 26.1 °C A) 0.0 °C B) 17.9 °C C) 11.6 °C D) -54.8 °C E) 26.1 °C

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

Which of the following reactions corresponds to the thermochemical equation for the standard molar enthalpy of formation of solid zinc nitrate?

(Multiple Choice)

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Question 41

The specific heat capacity of water(liquid)is 4.18 J/g⋅°C.What is the molar specific heat capacity of this substance? The molar mass of water is 18.01 g/mol.

(Multiple Choice)

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Question 42

Which one of the following statements is INCORRECT?

(Multiple Choice)

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Question 43

Many homes are heated using natural gas.The combustion of natural gas converts

(Multiple Choice)

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Question 44

What is the change in internal energy of the system (ΔU)if 65 kJ of heat energy is evolved by the system and 62 kJ of work is done on the system for a certain process?

(Multiple Choice)

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Question 45

CaO(s)reacts with water to form Ca(OH)₂(aq).If 6.50 g CaO is combined with 99.70 g H₂O in a coffee cup calorimeter,the temperature of the resulting solution increases from 21.7 °C to 43.1 °C.Calculate the enthalpy change for the reaction per mole of CaO.Assume that the specific heat capacity of the solution is 4.18 J/g⋅K.

(Multiple Choice)

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Question 46

What is the overall chemical equation that results from the sum of the given steps? 2 C(s)+ 2 H₂O(g)→ 2 CO(g)+ 2 H₂(g) CO(g)+ H₂O(g)→ CO₂(g)+ H₂(g) CO(g)+ 3 H₂(g)→ CH₄(g)+ H₂O(g)

(Multiple Choice)

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Question 47

When 1 mole of Fe₂O₃(s)reacts with H₂(g)to form Fe(s)and H₂O(g)by the following reaction,98.8 kJ of energy is absorbed. Fe₂O₃(s)+ 3 H₂(g)→ 2 Fe(s)+ 3 H₂O(g) (A) (B) Is the reaction endothermic or exothermic,and which of the enthalpy diagrams above Represents this reaction?

(Multiple Choice)

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Question 48

Specific heat capacity is

(Multiple Choice)

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Question 49

How much energy is needed to convert 50.8 g of ice at 0.00 °C to liquid water at 75.0 °C? Specific heat capacity (ice)= 2.10 J/g °C Specific heat capacity (liquid water)= 4.18 J/g °C Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g

(Multiple Choice)

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Question 50

Calculate the energy in the form of heat (in kJ)required to change 76.9 g of liquid water at 25.2 °C to ice at -15.2 °C.Assume that no energy in the form of heat is transferred to the environment.(Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06 J/g⋅K,liquid water = 4.184 J/g⋅K)

(Multiple Choice)

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Question 51

Which of the following has zero standard enthalpy of formation at 25 °C?

(Multiple Choice)

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Question 52

Combustion of 2.14 g of liquid benzene (C₆H₆)causes a temperature rise of 16.2 °C in a constant-pressure calorimeter that has a heat capacity of 5.53 kJ/°C.What is ΔH for the following reaction? C₆H₆(l)+ O₂(g)→ 6 CO₂(g)+ 3 H₂O( )

(Multiple Choice)

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Question 53

Determine the enthalpy change for the decomposition of calcium carbonate CaCO₃(s)→ CaO(s)+ CO₂(g) Given the thermochemical equations below. Ca(OH)₂(s)→ CaO(s)+ H₂O( ) Δ_rH° = 65.2 kJ/mol-rxn Ca(OH)₂(s)+ CO₂(g)→ CaCO₃(s)+ H₂O( ) Δ_rH° = −113.8 kJ/mol-rxn C(s)+ O₂(g)→ CO₂(g) Δ_rH° = −393.5 kJ/mol-rxn 2 Ca(s)+ O₂(g)→ 2 CaO(s) Δ_rH° = −1270.2 kJ/mol-rxn

(Multiple Choice)

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Question 54

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO₃(s)+ 2HCl(aq)→ CaCl₂(aq)+ H₂O(l)+ CO₂(g); Δ_rH° = -15.2 kJ/mol-rxn

(Multiple Choice)

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Question 55

Commercial cold packs consist of solid ammonium nitrate and water.NH₄NO₃ absorbs 25.69 kJ of heat per mole dissolved in water.In a coffee-cup calorimeter,5.60 g NH₄NO₃ is dissolved in 100.0 g of water at 22.0 °C.What is the final temperature of the solution? Assume that the solution has a specific heat capacity of 4.18 J/g⋅K.

(Multiple Choice)

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Question 56

When 50.0 mL of 1.60 M of HCl(aq)is combined with 50.0 mL of 1.70 M of NaOH(aq)in a coffee-cup calorimeter,the temperature of the solution increases by 10.7°C.What is the change in enthalpy for this balanced reaction? HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O( ) Assume that the solution density is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g⋅°C.

(Multiple Choice)

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Question 57

The energy associated with a stretched spring is called _____.

(Multiple Choice)

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Question 58

What quantity,in moles,of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H₂(g)and O₂(g)? H₂(g)+ O₂(g)→ H₂O(l); Δ_rH° = -285.8 kJ/mol-rxn

(Multiple Choice)

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Question 59

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H₂O(l)at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H₂O(l)is 4.18 J/(g·°C).

(Multiple Choice)

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Question 60

Showing 41 - 60 of 65

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

Which of the following reactions corresponds to the thermochemical equation for the standard molar enthalpy of formation of solid zinc nitrate?

The specific heat capacity of water(liquid)is 4.18 J/g⋅°C.What is the molar specific heat capacity of this substance? The molar mass of water is 18.01 g/mol.

Which one of the following statements is INCORRECT?

Many homes are heated using natural gas.The combustion of natural gas converts

What is the change in internal energy of the system (ΔU)if 65 kJ of heat energy is evolved by the system and 62 kJ of work is done on the system for a certain process?

What is the overall chemical equation that results from the sum of the given steps? ​ 2 C(s)+ 2 H2O(g)→ 2 CO(g)+ 2 H2(g) CO(g)+ H2O(g)→ CO2(g)+ H2(g) CO(g)+ 3 H2(g)→ CH4(g)+ H2O(g) ​

When 1 mole of Fe2O3(s)reacts with H2(g)to form Fe(s)and H2O(g)by the following reaction,98.8 kJ of energy is absorbed. Fe2O3(s)+ 3 H2(g)→ 2 Fe(s)+ 3 H2O(g) (A) (B) Is the reaction endothermic or exothermic,and which of the enthalpy diagrams above Represents this reaction?

Specific heat capacity is

How much energy is needed to convert 50.8 g of ice at 0.00 °C to liquid water at 75.0 °C? Specific heat capacity (ice)= 2.10 J/g °C Specific heat capacity (liquid water)= 4.18 J/g °C Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g

Which of the following has zero standard enthalpy of formation at 25 °C?

Combustion of 2.14 g of liquid benzene (C6H6)causes a temperature rise of 16.2 °C in a constant-pressure calorimeter that has a heat capacity of 5.53 kJ/°C.What is ΔH for the following reaction? C6H6(l)+ O2(g)→ 6 CO2(g)+ 3 H2O( )

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO3(s)+ 2HCl(aq)→ CaCl2(aq)+ H2O(l)+ CO2(g); ΔrH° = -15.2 kJ/mol-rxn

The energy associated with a stretched spring is called _____.

What quantity,in moles,of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H2(g)and O2(g)? H2(g)+ O2(g)→ H2O(l); ΔrH° = -285.8 kJ/mol-rxn

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H2O(l)at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H2O(l)is 4.18 J/(g·°C).

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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What is the overall chemical equation that results from the sum of the given steps? 2 C(s)+ 2 H₂O(g)→ 2 CO(g)+ 2 H₂(g) CO(g)+ H₂O(g)→ CO₂(g)+ H₂(g) CO(g)+ 3 H₂(g)→ CH₄(g)+ H₂O(g)

When 1 mole of Fe₂O₃(s)reacts with H₂(g)to form Fe(s)and H₂O(g)by the following reaction,98.8 kJ of energy is absorbed. Fe₂O₃(s)+ 3 H₂(g)→ 2 Fe(s)+ 3 H₂O(g) (A) (B) Is the reaction endothermic or exothermic,and which of the enthalpy diagrams above Represents this reaction?

Combustion of 2.14 g of liquid benzene (C₆H₆)causes a temperature rise of 16.2 °C in a constant-pressure calorimeter that has a heat capacity of 5.53 kJ/°C.What is ΔH for the following reaction? C₆H₆(l)+ O₂(g)→ 6 CO₂(g)+ 3 H₂O( )

How much heat is liberated at constant pressure if 0.515 g of calcium carbonate reacts with 32.7 mL of 0.498 M hydrochloric acid? CaCO₃(s)+ 2HCl(aq)→ CaCl₂(aq)+ H₂O(l)+ CO₂(g); Δ_rH° = -15.2 kJ/mol-rxn

What quantity,in moles,of hydrogen is consumed when 179.6 kJ of energy is evolved from the combustion of a mixture of H₂(g)and O₂(g)? H₂(g)+ O₂(g)→ H₂O(l); Δ_rH° = -285.8 kJ/mol-rxn

A 170.0-g sample of metal at 83.00°C is added to 170.0 g of H₂O(l)at 15.00°C in an insulated container.The temperature rises to 18.16°C.Neglecting the heat capacity of the container,what is the specific heat capacity of the metal? The specific heat capacity of H₂O(l)is 4.18 J/(g·°C).