Question 1

The only way in which a system can do work on the surroundings is by expansion against the external pressure.

Accepted Answer

A) True 
 B)False

Question 2

A 275-g sample of nickel at l00.0°C is placed in 100.0 mL of water at 22.0°C.What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings.Specific heat capacity of nickel = 0.444 J/(g·K)

Accepted Answer

A) 39.6°C 
B) 40.8°C 
C) 61.0°C 
D) 79.2°C 
E) 82.4°C 
A) 39.6°C 
B) 40.8°C 
C) 61.0°C 
D) 79.2°C 
E) 82.4°C

Question 3

The highly exothermic thermite reaction,in which aluminum reduces iron(III)oxide to elemental iron,has been used by railroad repair crews to weld rails together.
 
What mass of iron is formed when 725 kJ of heat are released?

Accepted Answer

A) 47 g 
B) 65 g 
C) 95 g 
D) 112 g 
E) 130 g 
A) 47 g 
B) 65 g 
C) 95 g 
D) 112 g 
E) 130 g

Question 4

a.State Hess's Law.
b.Use the $\Delta$H° data given below to calculate $\Delta$H° for the reaction:
C2H4(g)+ H2(g) $\to$ C2H6(g)
Data:

Accepted Answer

a.The enthalpy change for an o

Question 5

Ethanol,C2H5OH,is being promoted as a clean fuel and is used as an additive in many gasoline mixtures.Calculate the $\Delta$H°rxn for the combustion of ethanol.$\Delta$H°f [C2H5OH(l)] = -277.7 kJ/mol;
$\Delta$H°f [CO2(g)] = -393.5 kJ/mol;$\Delta$H°f [H2O(g)] = -241.8 kJ/mol

Accepted Answer

A) -1234.7 kJ 
B) -751.1 kJ 
C) -357.6 kJ 
D) 357.6 kJ 
E) 1234.7 kJ 
A) -1234.7 kJ 
B) -751.1 kJ 
C) -357.6 kJ 
D) 357.6 kJ 
E) 1234.7 kJ

Question 6

Use the following data to calculate the standard heat (enthalpy)of formation,$\Delta$H°f ,of manganese(IV)oxide,MnO2 (s).

Accepted Answer

A) -504 kJ 
B) -372 kJ 
C) -24 kJ 
D) 24 kJ 
E) 504 kJ 
A) -504 kJ 
B) -372 kJ 
C) -24 kJ 
D) 24 kJ 
E) 504 kJ

Question 7

In an endothermic reaction,in going from the reactants to the products at the same temperature,the value of q is negative.

Accepted Answer

A) True 
 B)False

Question 8

Your favorite candy bar,Gummy Beakers,contains 1.2 $\times$ 106 J of energy while your favorite soft drink,Bolt,contains 6.7 $\times$ 105 J.If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt,what percent of your 2000 Calorie daily food intake is left for broccoli,beans,beef,etc.?

Accepted Answer

A) 53% 
B) 47% 
C) 27% 
D) 11% 
E) 0% 
A) 53% 
B) 47% 
C) 27% 
D) 11% 
E) 0%

Question 9

Different chemical bonds have different potential energies.

Accepted Answer

A) True 
 B)False

Question 10

Ethylene glycol,used as a coolant in automotive engines,has a specific heat capacity of 2.42 J/(g·K).Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C.

Accepted Answer

A) -1900 kJ 
B) -420 kJ 
C) -99 kJ 
D) -0.42 kJ 
E) -4.2 $\times$ 10-6 kJ 
A) -1900 kJ 
B) -420 kJ 
C) -99 kJ 
D) -0.42 kJ 
E) -4.2 $\times$ 10-6 kJ

Question 11

A system which undergoes an adiabatic change and does work on the surroundings has

Accepted Answer

A) w 0,$\Delta$E > 0 C) w > 0,$\Delta$E 0 E) w < 0,$\Delta$E < 0 A) w 0,$\Delta$E > 0 C) w > 0,$\Delta$E 0 E) w < 0,$\Delta$E < 0

Question 12

Use Hess's Law to calculate the enthalpy change for the reaction
WO3(s)+ 3H2(g) $\to$ W(s)+ 3H2O(g)
From the following data:

Accepted Answer

A) 125.9 kJ 
B) 252.9 kJ 
C) 364.9 kJ 
D) 1207.6 kJ 
E) None of these choices is correct. 
A) 125.9 kJ 
B) 252.9 kJ 
C) 364.9 kJ 
D) 1207.6 kJ 
E) None of these choices is correct.

Question 13

Calculate the $\Delta$H°rxn for the following reaction.$\Delta$H°f [SiO2(s)] = -910.9 kJ/mol;F$\Delta$H°f [SiCl4(g)] = -657.0 kJ/mol;$\Delta$H°f [HCl(g)] = -92.3 kJ/mol;$\Delta$H°f [H2O (g)] = -241.8 kJ/mol
SiO2(s)+ 4HCl(g) $\to$ SiCl4(g)+ 2H2O(g)

Accepted Answer

A) -139.5 kJ 
B) -137.4 kJ 
C) -104.4 kJ 
D) 104.4 kJ 
E) 139.5 kJ 
A) -139.5 kJ 
B) -137.4 kJ 
C) -104.4 kJ 
D) 104.4 kJ 
E) 139.5 kJ

Question 14

A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings.If the initial internal energy,E,is 61.2 kJ,what is the final value of E?

Accepted Answer

A) 32.7 kJ 
B) 46.5 kJ 
C) 75.9 kJ 
D) 82.8 kJ 
E) 89.7 kJ 
A) 32.7 kJ 
B) 46.5 kJ 
C) 75.9 kJ 
D) 82.8 kJ 
E) 89.7 kJ

Question 15

If,as a pioneer,you wished to warm your room by taking an object heated on top of a pot-bellied stove to it,which of the following 15-pound objects,each heated to 100°C,would be the best choice? The specific heat capacity (in J/(g·K))for each substance is given in parentheses.Iron (0.450),copper (0.387),granite (0.79),gold (0.129),water (4.18).

Accepted Answer

A) iron 
B) copper 
C) granite 
D) gold 
E) water 
A) iron 
B) copper 
C) granite 
D) gold 
E) water

Question 16

Which one of the following is not a correct formation reaction? (products are correct)

Accepted Answer

A) H2(g)+ O(g) $\to$ H2O(l) 
B) 
 
H2(g)+
 
Cl2(g) $\to$ HCl(g) 
C) 6C(graphite)+ 3H2(g) $\to$ C6H6(l) 
D) C(graphite) $\to$ C(diamond) 
E) 6C(graphite)+ 6H2(g)+ 3O2(g) $\to$C6H12O6(s) 
A) H2(g)+ O(g) $\to$ H2O(l) 
B) 
 
H2(g)+
 
Cl2(g) $\to$ HCl(g) 
C) 6C(graphite)+ 3H2(g) $\to$ C6H6(l) 
D) C(graphite) $\to$ C(diamond) 
E) 6C(graphite)+ 6H2(g)+ 3O2(g) $\to$C6H12O6(s)

Question 17

$\Delta$H does not depend on the path of a reaction,but $\Delta$E does.

Accepted Answer

A) True 
 B)False

Question 18

Given the following data:
   
calculate $\Delta$H° for the reaction
NO(g)+ O(g)$\to$NO2(g)

Accepted Answer

The answer of Given the following data:
   
calculate...

Question 19

a.Write a balanced equation for the combustion of benzene,C6H6(l)in oxygen.
b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation,$\Delta$H°f ,given the data:
$\Delta$H°f [CO2(g)] = -394 kJ;$\Delta$H°f [H2O(l)] = -286 kJ

Accepted Answer

a.C₆H₆(l

Question 20

Galena is the ore from which elemental lead is extracted.In the first step of the extraction process,galena is heated in air to form lead(II)oxide.
 
What mass of galena is converted to lead oxide if 975 kJ of heat are liberated?

Accepted Answer

A) 203 g 
B) 282 g 
C) 406 g 
D) 478 g 
E) 564 g 
A) 203 g 
B) 282 g 
C) 406 g 
D) 478 g 
E) 564 g

The only way in which a system can do work on the surroundings is by expansion against the external pressure.

A 275-g sample of nickel at l00.0°C is placed in 100.0 mL of water at 22.0°C.What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings.Specific heat capacity of nickel = 0.444 J/(g·K)

The highly exothermic thermite reaction,in which aluminum reduces iron(III)oxide to elemental iron,has been used by railroad repair crews to weld rails together. What mass of iron is formed when 725 kJ of heat are released?

Ethanol,C₂H₅OH,is being promoted as a clean fuel and is used as an additive in many gasoline mixtures.Calculate the $\Delta$ H°_rxn for the combustion of ethanol. $\Delta$ H°_f [C₂H₅OH(l)] = -277.7 kJ/mol; $\Delta$ H°_f [CO₂(g)] = -393.5 kJ/mol; $\Delta$ H°_f [H₂O(g)] = -241.8 kJ/mol

Use the following data to calculate the standard heat (enthalpy)of formation, $\Delta$ H°_f ,of manganese(IV)oxide,MnO₂ (s). $Use the following data to calculate the standard heat (enthalpy)of formation, \Delta H°<sub>f</sub> ,of manganese(IV)oxide,MnO<sub>2</sub> (s).$

In an endothermic reaction,in going from the reactants to the products at the same temperature,the value of q is negative.

Different chemical bonds have different potential energies.

Ethylene glycol,used as a coolant in automotive engines,has a specific heat capacity of 2.42 J/(g·K).Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C.

A system which undergoes an adiabatic change and does work on the surroundings has

Use Hess's Law to calculate the enthalpy change for the reaction WO₃(s)+ 3H₂(g) $\to$ W(s)+ 3H₂O(g) From the following data: $Use Hess's Law to calculate the enthalpy change for the reaction WO<sub>3</sub>(s)+ 3H<sub>2</sub>(g) \to W(s)+ 3H<sub>2</sub>O(g) From the following data:$

Calculate the $\Delta$ H°_rxn for the following reaction. $\Delta$ H°_f [SiO₂(s)] = -910.9 kJ/mol;F $\Delta$ H°_f [SiCl₄(g)] = -657.0 kJ/mol; $\Delta$ H°_f [HCl(g)] = -92.3 kJ/mol; $\Delta$ H°_f [H₂O (g)] = -241.8 kJ/mol SiO₂(s)+ 4HCl(g) $\to$ SiCl₄(g)+ 2H₂O(g)

A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings.If the initial internal energy,E,is 61.2 kJ,what is the final value of E?

Which one of the following is not a correct formation reaction? (products are correct)

$\Delta$ H does not depend on the path of a reaction,but $\Delta$ E does.

Given the following data: $Given the following data: calculate \Delta H° for the reaction NO(g)+ O(g) \to NO<sub>2</sub>(g)$ calculate $\Delta$ H° for the reaction NO(g)+ O(g) $\to$ NO₂(g)

a.Write a balanced equation for the combustion of benzene,C₆H₆(l)in oxygen. b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation, $\Delta$ H°_f ,given the data: $\Delta$ H°_f [CO₂(g)] = -394 kJ; $\Delta$ H°_f [H₂O(l)] = -286 kJ

Galena is the ore from which elemental lead is extracted.In the first step of the extraction process,galena is heated in air to form lead(II)oxide. What mass of galena is converted to lead oxide if 975 kJ of heat are liberated?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 6: Thermochemistry: Energy Flow and Chemical Change

The only way in which a system can do work on the surroundings is by expansion against the external pressure.

A 275-g sample of nickel at l00.0°C is placed in 100.0 mL of water at 22.0°C.What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings.Specific heat capacity of nickel = 0.444 J/(g·K)

The highly exothermic thermite reaction,in which aluminum reduces iron(III)oxide to elemental iron,has been used by railroad repair crews to weld rails together. What mass of iron is formed when 725 kJ of heat are released?

a.State Hess's Law. b.Use the Δ\DeltaΔ H° data given below to calculate Δ\DeltaΔ H° for the reaction: C2H4(g)+ H2(g) →\to→ C2H6(g) Data:

Ethanol,C2H5OH,is being promoted as a clean fuel and is used as an additive in many gasoline mixtures.Calculate the Δ\DeltaΔ H°rxn for the combustion of ethanol. Δ\DeltaΔ H°f [C2H5OH(l)] = -277.7 kJ/mol; Δ\DeltaΔ H°f [CO2(g)] = -393.5 kJ/mol; Δ\DeltaΔ H°f [H2O(g)] = -241.8 kJ/mol

Use the following data to calculate the standard heat (enthalpy)of formation, Δ\DeltaΔ H°f ,of manganese(IV)oxide,MnO2 (s).

In an endothermic reaction,in going from the reactants to the products at the same temperature,the value of q is negative.

Different chemical bonds have different potential energies.

Ethylene glycol,used as a coolant in automotive engines,has a specific heat capacity of 2.42 J/(g·K).Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C.

A system which undergoes an adiabatic change and does work on the surroundings has

Use Hess's Law to calculate the enthalpy change for the reaction WO3(s)+ 3H2(g) →\to→ W(s)+ 3H2O(g) From the following data:

Calculate the Δ\DeltaΔ H°rxn for the following reaction. Δ\DeltaΔ H°f [SiO2(s)] = -910.9 kJ/mol;F Δ\DeltaΔ H°f [SiCl4(g)] = -657.0 kJ/mol; Δ\DeltaΔ H°f [HCl(g)] = -92.3 kJ/mol; Δ\DeltaΔ H°f [H2O (g)] = -241.8 kJ/mol SiO2(s)+ 4HCl(g) →\to→ SiCl4(g)+ 2H2O(g)

A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings.If the initial internal energy,E,is 61.2 kJ,what is the final value of E?

Which one of the following is not a correct formation reaction? (products are correct)

Δ\DeltaΔ H does not depend on the path of a reaction,but Δ\DeltaΔ E does.

Given the following data: calculate Δ\DeltaΔ H° for the reaction NO(g)+ O(g) →\to→ NO2(g)

a.Write a balanced equation for the combustion of benzene,C6H6(l)in oxygen. b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation, Δ\DeltaΔ H°f ,given the data: Δ\DeltaΔ H°f [CO2(g)] = -394 kJ; Δ\DeltaΔ H°f [H2O(l)] = -286 kJ

Galena is the ore from which elemental lead is extracted.In the first step of the extraction process,galena is heated in air to form lead(II)oxide. What mass of galena is converted to lead oxide if 975 kJ of heat are liberated?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids,solids,and Phase Changes

The Properties of Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Use the following data to calculate the standard heat (enthalpy)of formation, $\Delta$ H°_f ,of manganese(IV)oxide,MnO₂ (s). $Use the following data to calculate the standard heat (enthalpy)of formation, \Delta H°<sub>f</sub> ,of manganese(IV)oxide,MnO<sub>2</sub> (s).$

Use Hess's Law to calculate the enthalpy change for the reaction WO₃(s)+ 3H₂(g) $\to$ W(s)+ 3H₂O(g) From the following data: $Use Hess's Law to calculate the enthalpy change for the reaction WO<sub>3</sub>(s)+ 3H<sub>2</sub>(g) \to W(s)+ 3H<sub>2</sub>O(g) From the following data:$

Calculate the $\Delta$ H°_rxn for the following reaction. $\Delta$ H°_f [SiO₂(s)] = -910.9 kJ/mol;F $\Delta$ H°_f [SiCl₄(g)] = -657.0 kJ/mol; $\Delta$ H°_f [HCl(g)] = -92.3 kJ/mol; $\Delta$ H°_f [H₂O (g)] = -241.8 kJ/mol SiO₂(s)+ 4HCl(g) $\to$ SiCl₄(g)+ 2H₂O(g)

$\Delta$ H does not depend on the path of a reaction,but $\Delta$ E does.

Given the following data: $Given the following data: calculate \Delta H° for the reaction NO(g)+ O(g) \to NO<sub>2</sub>(g)$ calculate $\Delta$ H° for the reaction NO(g)+ O(g) $\to$ NO₂(g)

a.Write a balanced equation for the combustion of benzene,C₆H₆(l)in oxygen. b.The standard heat of combustion of benzene is -3271 kJ/mol.Calculate its standard heat of formation, $\Delta$ H°_f ,given the data: $\Delta$ H°_f [CO₂(g)] = -394 kJ; $\Delta$ H°_f [H₂O(l)] = -286 kJ