Question 1

Use the following data to calculate the standard heat (enthalpy) of formation, Δ\DeltaΔ H°f ,of manganese(IV) oxide,MnO2 (s) .
f ,of manganese(IV) oxide,MnO2 (s) .   A) -504 kJ B) -372 kJ C) -24 kJ D) 24 kJ E) 504 kJ " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  -504 kJ
B)  -372 kJ
C)  -24 kJ
D)  24 kJ
E)  504 kJ F) A) and B)
G) None of the above

Question 2

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 3

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 4

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

Accepted Answer

A)  w Δ\DeltaΔ E = 0
B)  w > 0, Δ\DeltaΔ E > 0
C)  w > 0, Δ\DeltaΔ E 
D)  w Δ\DeltaΔ E > 0
E)  w Δ\DeltaΔ E < 0 F) C) and D)
G) C) and E)

Question 5

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°CF) B) and D)
G) A) and B)

Question 6

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

Accepted Answer

A) True 
 B)False

Question 7

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 gF) B) and D)
G) A) and D)

Question 8

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

Accepted Answer

A)  -1234.7 kJ
B)  -751.1 kJ
C)  -357.6 kJ
D)  357.6 kJ
E)  1234.7 kJ F) All of the above
G) None of the above

Question 9

Use Hess's Law to calculate the enthalpy change for the reaction
WO3(s) + 3H2(g)   →	o→  W(s) + 3H2O(g) 
From the following data:
3(s) + 3H2(g)   	o  W(s) + 3H2O(g)  From the following data:   A) 125.9 kJ B) 252.9 kJ C) 364.9 kJ D) 1207.6 kJ E) None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" >

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. F) C) and D)
G) None of the above

Question 10

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 gF) A) and B)
G) D) and E)

Question 11

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 $\Delta$H°...

Question 12

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 kJF) A) and E)
G) C) and D)

Question 13

Your favorite candy bar,Gummy Beakers,contains 1.2  ×	imes×  106 J of energy while your favorite soft drink,Bolt,contains 6.7  ×	imes×  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% F) A) and D)
G) B) and C)

Question 14

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)   →	o→  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 F) All of the above
G) A) and E)

Question 15

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

Accepted Answer

A)  H2(g) + O(g)   →	o→  H2O(l) 
B)  2(g) + O(g)   	o  H2O(l)  
B)     H2(g) +   Cl2(g)   	o  HCl(g)  
C)  6C(graphite) + 3H2(g)   	o  C6H6(l)  
D)  C(graphite)   	o  C(diamond)  
E)  6C(graphite) + 6H2(g) + 3O2(g)   	o C6H12O6(s)  " class="answers-bank-image d-inline" rel="preload" >H2(g) +2(g) + O(g)   	o  H2O(l)  
B)     H2(g) +   Cl2(g)   	o  HCl(g)  
C)  6C(graphite) + 3H2(g)   	o  C6H6(l)  
D)  C(graphite)   	o  C(diamond)  
E)  6C(graphite) + 6H2(g) + 3O2(g)   	o C6H12O6(s)  " class="answers-bank-image d-inline" rel="preload" >Cl2(g)   →	o→  HCl(g) 
C)  6C(graphite) + 3H2(g)   →	o→  C6H6(l) 
D)  C(graphite)   →	o→  C(diamond) 
E)  6C(graphite) + 6H2(g) + 3O2(g)   →	o→ C6H12O6(s)  F) B) and C)
G) B) and E)

Question 16

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  ×	imes×  10-6 kJ F) A) and B)
G) A) and C)

Question 17

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 18

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)  waterF) A) and B)
G) A) and C)

Question 19

Different chemical bonds have different potential energies.

Accepted Answer

A) True 
 B)False

Question 20

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...

Exam 6: Thermochemistry: Energy Flow and Chemical Change

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?

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

Different chemical bonds have different potential energies.

Correct Answer
verified

Correct Answer
verified
a.The enthalpy change for an o...
View Answer

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
a.C₆H₆(l...
View Answer

Correct Answer
verified

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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.

Correct Answer
verified

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?

Correct Answer
verified

Exam 6: Thermochemistry: Energy Flow and Chemical Change

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Different chemical bonds have different potential energies.

Correct AnswerverifiedShow Answer

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:

Correct Answerverifieda.The enthalpy change for an o...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct Answerverifieda.C6H6(l...View AnswerShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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:

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
a.The enthalpy change for an o...
View Answer

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified
a.C₆H₆(l...
View Answer

Correct Answer
verified

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified