Question 1

Which of the following are thermodynamic state functions?
I.heat
II.volume
III.temperature
IV.enthalpy
V.density

Accepted Answer

A) II,III,IV,V 
B) I,II,IV,V 
C) I,II,III,V 
D) II,IV 
E) I,III,V 
A) II,III,IV,V 
B) I,II,IV,V 
C) I,II,III,V 
D) II,IV 
E) I,III,V

Question 2

Calculate the quantity of heat,in kJ,required to raise the temperature of a 2.15 kg iron bar 24.0 °C (specific heat of iron = 0.473 J/g °C).

Accepted Answer

A) 109 kJ 
B) 51.6 kJ 
C) 23.6 kJ 
D) 24.4 kJ 
E) 11.3 kJ 
A) 109 kJ 
B) 51.6 kJ 
C) 23.6 kJ 
D) 24.4 kJ 
E) 11.3 kJ

Question 3

A system absorbs 623 J of heat while doing 457 J of work.What is the value of ΔU?

Accepted Answer

A) +1080 J 
B) -166 J 
C) +166 J 
D) -1080 J 
E) +623 J 
A) +1080 J 
B) -166 J 
C) +166 J 
D) -1080 J 
E) +623 J

Question 4

At 1.0133 bar,the heat of sublimation of gallium is 277 kJ mol-1 And the heat of vaporization is 271 kJ mol-1 .To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1.0133 bar?

Accepted Answer

A) 6 kJ 
B) 33 kJ 
C) 244 kJ 
D) 274 kJ 
A) 6 kJ 
B) 33 kJ 
C) 244 kJ 
D) 274 kJ

Question 5

The complete combustion of propane,C3H8(g),is represented by the equation:
C3H8(g)+ 5 O2(g)→ 3 CO2(g)+ 4 H2O(l)ΔrH° = -2220 kJ /mol
How much heat is evolved in the complete combustion of 20.0 L C3H8(g)at STP?

Accepted Answer

A) 2486 kJ 
B) 1007 kJ 
C) 994 kJ 
D) 1957 kJ 
E) 495 kJ 
A) 2486 kJ 
B) 1007 kJ 
C) 994 kJ 
D) 1957 kJ 
E) 495 kJ

Question 6

Many people believe that coffee  
May be cooled by placing a silver spoon  
In the coffee.If 250 ml  
Of coffee at 200 °F had a spoon at 70 °F placed in it,what would be the final Celsius temperature of the spoon and coffee,assuming that no heat is lost to the surroundings? The mass of the spoon is 35 g.

Accepted Answer

A) 92.8 °C 
B) 72.2 °C 
C) 57.2 °C 
D) 82.0 °C 
E) 199 °C 
A) 92.8 °C 
B) 72.2 °C 
C) 57.2 °C 
D) 82.0 °C 
E) 199 °C

Question 7

Given the following reactions:
2 NOCl(g)→ 2 NO(g)+ Cl2(g)ΔrH° = +75.56 kJ/mol
2 NO(g)+ O2(g)→ 2 NO2(g)ΔrH° = -113.05 kJ/mol
2 NO2(g)→ N2O4(g)ΔrH° = -58.03 kJ/mol
Compute ΔrH° of N2O4(g)+ Cl2(g)→ 2 NOCl(g)+ O2(g)in kJ/mol.

Accepted Answer

A) +246.65 kJ/mol 
B) -95.52 kJ/mol 
C) -246.65 kJ/mol 
D) +95.52 kJ/mol 
E) +130.58 kJ/mol 
A) +246.65 kJ/mol 
B) -95.52 kJ/mol 
C) -246.65 kJ/mol 
D) +95.52 kJ/mol 
E) +130.58 kJ/mol

Question 8

100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0 °C.The final temperature of the nickel-water mixture was 26.3 °C.What is the specific heat of the nickel?

Accepted Answer

A) 0.14 J/g °C 
B) 0.13 J/g °C 
C) 0.55 J/g °C 
D) 0.44 J/g °C 
E) 0.23 J/g °C 
A) 0.14 J/g °C 
B) 0.13 J/g °C 
C) 0.55 J/g °C 
D) 0.44 J/g °C 
E) 0.23 J/g °C

Question 9

Determine the enthalpy change in the following equation:

Accepted Answer

A) -562 kJ/mol 
B) -375 kJ/mol 
C) 375 kJ /mol 
D) -402 kJ/mol 
E) 402 kJ/mol 
A) -562 kJ/mol 
B) -375 kJ/mol 
C) 375 kJ /mol 
D) -402 kJ/mol 
E) 402 kJ/mol

Question 10

For the reaction H2(g)+ 1/2 O2(g)→ H2O(g)ΔrH° = -241.8 kJ/mol,
What quantity of heat,in kJ,evolved when a 72.0 g mixture containing equal parts of H2 and O2,by mass,is burned?

Accepted Answer

A) 8630 kJ 
B) 4860 kJ 
C) 1088 kJ 
D) 272 kJ 
E) 544 kJ 
A) 8630 kJ 
B) 4860 kJ 
C) 1088 kJ 
D) 272 kJ 
E) 544 kJ

Question 11

500 g of Al is heated to 100.0 °C and dropped into a l00.0 g glass beaker that contains 200.0 g of H2O.The temperature of the glass and water is 20.0 °C.What is the final temperature? (Specific heat of Al = 0.29 J/g °C,specific heat of glass = 0.84 J/g °C)

Accepted Answer

A) 46.6 °C 
B) 50.0 °C 
C) 25.0 °C 
D) 30.9 °C 
E) 28.9 °C 
A) 46.6 °C 
B) 50.0 °C 
C) 25.0 °C 
D) 30.9 °C 
E) 28.9 °C

Question 12

1674 J of heat are absorbed by 25.0 mL of NaOH (d = 1.10 g/mL,specific heat = 4.10 J/g °C).The temperature of the NaOH goes up by how many degrees?

Accepted Answer

A) 14.8 °C 
B) 18.0 °C 
C) 17.2 °C 
D) 14.2 °C 
E) 19.1 °C 
A) 14.8 °C 
B) 18.0 °C 
C) 17.2 °C 
D) 14.2 °C 
E) 19.1 °C

Question 13

What is the reaction for the standard enthalpy of formation for Mn2O3(s)? 
(Mn(s)is the stable form of manganese. )

Accepted Answer

A) Mn(s)+ 3/4 O2(g)→ 1/2 Mn2O3(s) 
B) MnO(s)+ MnO2(s)→ Mn2O3(s) 
C) 2 Mn(s)+ O3(g)→ Mn2O3(s) 
D) 2 MnO(s)+ 1/2 O3(g)→ Mn2O3(s) 
E) 2Mn (s)+ 3/2 O2 (g)→ Mn2O3(s) 
A) Mn(s)+ 3/4 O2(g)→ 1/2 Mn2O3(s) 
B) MnO(s)+ MnO2(s)→ Mn2O3(s) 
C) 2 Mn(s)+ O3(g)→ Mn2O3(s) 
D) 2 MnO(s)+ 1/2 O3(g)→ Mn2O3(s) 
E) 2Mn (s)+ 3/2 O2 (g)→ Mn2O3(s)

Question 14

1219 joules of heat raise the temperature of 250 g of metal by 64 °C.What is the specific heat of the metal in J/(g °C?)

Accepted Answer

A) (1219)(250)(64)J/(g °
C)  
B) (64)(250/1219)J/(g °
C)  
C) (1219)(64/250)J/(g °
C)  
D) (1219)(250/64)J/(g °
C)  
E) (1219)/(250 × 64)J/(g °
C)  
A) (1219)(250)(64)J/(g °
C)  
B) (64)(250/1219)J/(g °
C)  
C) (1219)(64/250)J/(g °
C)  
D) (1219)(250/64)J/(g °
C)  
E) (1219)/(250 × 64)J/(g °
C)

Question 15

Complete combustion of 75.0 g acetylene,C2H2,liberated 3750 kJ of heat.What is the heat of combustion,ΔrHcomb,of acetylene?

Accepted Answer

A) -50.0 kJ/mol 
B) +50.0 kJ/mol 
C) +1302 kJ/mol 
D) -1302 kJ/mol 
E) -0.521 kJ/mol 
A) -50.0 kJ/mol 
B) +50.0 kJ/mol 
C) +1302 kJ/mol 
D) -1302 kJ/mol 
E) -0.521 kJ/mol

Question 16

2 LiOH(s)→ Li2O(s)+ H2O(l)ΔrH° = 379.1 kJ/mol
LiH(s)+ H2O(l)→ LiOH(s)+ H2(g)ΔrH° = -111.0 kJ/mol
2 H2(g)+ O2(g)→ 2 H2O(l)ΔrH° = -285.9 kJmol
Compute ΔrH° in kJ/mol for 2 LiH(s)+ O2(g)→ Li2O(s)+ H2O(l)

Accepted Answer

A) +125.2 kJ/mol 
B) -17.7 kJ/mol 
C) -128.8 kJ/mol 
D) -303.6 kJ/mol 
E) + 128.8 kJ/mol 
A) +125.2 kJ/mol 
B) -17.7 kJ/mol 
C) -128.8 kJ/mol 
D) -303.6 kJ/mol 
E) + 128.8 kJ/mol

Question 17

Determine the enthalpy change in the following equation:
2 NH3(g)→ N2(g)+ 3 H2(g)
ΔfH° NH3(g)= -46.11 kJ/mol

Accepted Answer

A) 92.22 kJ/mol 
B) 46.11 kJ/mol 
C) 5.42 kJ/mol 
D) -92.22 kJ/mol 
E) -46.11 kJ/mol 
A) 92.22 kJ/mol 
B) 46.11 kJ/mol 
C) 5.42 kJ/mol 
D) -92.22 kJ/mol 
E) -46.11 kJ/mol

Question 18

Which of the following has a standard enthalpy of formation of zero?

Accepted Answer

A) Ar(g) 
B) I2(g) 
C) Br2(g) 
D) O3(g) 
E) P(s,red) 
A) Ar(g) 
B) I2(g) 
C) Br2(g) 
D) O3(g) 
E) P(s,red)

Question 19

Given the following thermochemical equations:
 
Compute the ΔfH° for FeS2(s)in kJ/mol.

Accepted Answer

A) -1233.9 kJ/mol 
B) -2893.9 kJ/mol 
C) -24.3 kJ/mol 
D) -183.5 kJ/mol 
E) -70.0 kJ/mol 
A) -1233.9 kJ/mol 
B) -2893.9 kJ/mol 
C) -24.3 kJ/mol 
D) -183.5 kJ/mol 
E) -70.0 kJ/mol

Question 20

The heat of combustion of methane is -50.38 kJ/mol.How many moles of methane must be burned to produce 137 kJ of heat?

Accepted Answer

A) 6.90 mol 
B) 0.367 mol 
C) 2.72 mol 
D) 1.37 mol 
E) 0.272 mol 
A) 6.90 mol 
B) 0.367 mol 
C) 2.72 mol 
D) 1.37 mol 
E) 0.272 mol

Exam 7: Thermochemistry

Which of the following are thermodynamic state functions? I.heat II.volume III.temperature IV.enthalpy V.density

Calculate the quantity of heat,in kJ,required to raise the temperature of a 2.15 kg iron bar 24.0 °C (specific heat of iron = 0.473 J/g °C).

A system absorbs 623 J of heat while doing 457 J of work.What is the value of ΔU?

At 1.0133 bar,the heat of sublimation of gallium is 277 kJ mol-1 And the heat of vaporization is 271 kJ mol-1 .To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1.0133 bar?

The complete combustion of propane,C3H8(g),is represented by the equation: C3H8(g)+ 5 O2(g)→ 3 CO2(g)+ 4 H2O(l)ΔrH° = -2220 kJ /mol How much heat is evolved in the complete combustion of 20.0 L C3H8(g)at STP?

Given the following reactions: 2 NOCl(g)→ 2 NO(g)+ Cl2(g)ΔrH° = +75.56 kJ/mol 2 NO(g)+ O2(g)→ 2 NO2(g)ΔrH° = -113.05 kJ/mol 2 NO2(g)→ N2O4(g)ΔrH° = -58.03 kJ/mol Compute ΔrH° of N2O4(g)+ Cl2(g)→ 2 NOCl(g)+ O2(g)in kJ/mol.

100.0 g of nickel at 150 °C was placed in 1.00 L of water at 25.0 °C.The final temperature of the nickel-water mixture was 26.3 °C.What is the specific heat of the nickel?

Determine the enthalpy change in the following equation:

For the reaction H2(g)+ 1/2 O2(g)→ H2O(g)ΔrH° = -241.8 kJ/mol, What quantity of heat,in kJ,evolved when a 72.0 g mixture containing equal parts of H2 and O2,by mass,is burned?

500 g of Al is heated to 100.0 °C and dropped into a l00.0 g glass beaker that contains 200.0 g of H2O.The temperature of the glass and water is 20.0 °C.What is the final temperature? (Specific heat of Al = 0.29 J/g °C,specific heat of glass = 0.84 J/g °C)

1674 J of heat are absorbed by 25.0 mL of NaOH (d = 1.10 g/mL,specific heat = 4.10 J/g °C).The temperature of the NaOH goes up by how many degrees?

What is the reaction for the standard enthalpy of formation for Mn2O3(s)? (Mn(s)is the stable form of manganese. )

1219 joules of heat raise the temperature of 250 g of metal by 64 °C.What is the specific heat of the metal in J/(g °C?)

Complete combustion of 75.0 g acetylene,C2H2,liberated 3750 kJ of heat.What is the heat of combustion,ΔrHcomb,of acetylene?

2 LiOH(s)→ Li2O(s)+ H2O(l)ΔrH° = 379.1 kJ/mol LiH(s)+ H2O(l)→ LiOH(s)+ H2(g)ΔrH° = -111.0 kJ/mol 2 H2(g)+ O2(g)→ 2 H2O(l)ΔrH° = -285.9 kJmol Compute ΔrH° in kJ/mol for 2 LiH(s)+ O2(g)→ Li2O(s)+ H2O(l)

Determine the enthalpy change in the following equation: 2 NH3(g)→ N2(g)+ 3 H2(g) ΔfH° NH3(g)= -46.11 kJ/mol

Which of the following has a standard enthalpy of formation of zero?

Given the following thermochemical equations: Compute the ΔfH° for FeS2(s)in kJ/mol.

The heat of combustion of methane is -50.38 kJ/mol.How many moles of methane must be burned to produce 137 kJ of heat?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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At 1.0133 bar,the heat of sublimation of gallium is 277 kJ mol^-1 And the heat of vaporization is 271 kJ mol^-1 .To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1.0133 bar?

The complete combustion of propane,C₃H₈(g),is represented by the equation: C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4 H₂O(l)Δ_rH° = -2220 kJ /mol How much heat is evolved in the complete combustion of 20.0 L C₃H₈(g)at STP?

Given the following reactions: 2 NOCl(g)→ 2 NO(g)+ Cl₂(g)Δ_rH° = +75.56 kJ/mol 2 NO(g)+ O₂(g)→ 2 NO₂(g)Δ_rH° = -113.05 kJ/mol 2 NO₂(g)→ N₂O₄(g)Δ_rH° = -58.03 kJ/mol Compute Δ_rH° of N₂O₄(g)+ Cl₂(g)→ 2 NOCl(g)+ O₂(g)in kJ/mol.

For the reaction H₂(g)+ 1/2 O₂(g)→ H₂O(g)Δ_rH° = -241.8 kJ/mol, What quantity of heat,in kJ,evolved when a 72.0 g mixture containing equal parts of H₂ and O₂,by mass,is burned?

500 g of Al is heated to 100.0 °C and dropped into a l00.0 g glass beaker that contains 200.0 g of H₂O.The temperature of the glass and water is 20.0 °C.What is the final temperature? (Specific heat of Al = 0.29 J/g °C,specific heat of glass = 0.84 J/g °C)

What is the reaction for the standard enthalpy of formation for Mn₂O₃(s)? (Mn(s)is the stable form of manganese. )

Complete combustion of 75.0 g acetylene,C₂H₂,liberated 3750 kJ of heat.What is the heat of combustion,Δ_rH_comb,of acetylene?

2 LiOH(s)→ Li₂O(s)+ H₂O(l)Δ_rH° = 379.1 kJ/mol LiH(s)+ H₂O(l)→ LiOH(s)+ H₂(g)Δ_rH° = -111.0 kJ/mol 2 H₂(g)+ O₂(g)→ 2 H₂O(l)Δ_rH° = -285.9 kJmol Compute Δ_rH° in kJ/mol for 2 LiH(s)+ O₂(g)→ Li₂O(s)+ H₂O(l)

Determine the enthalpy change in the following equation: 2 NH₃(g)→ N₂(g)+ 3 H₂(g) Δ_fH° NH₃(g)= -46.11 kJ/mol

Given the following thermochemical equations: Compute the Δ_fH° for FeS₂(s)in kJ/mol.