Question 1

The standard enthalpy of formation of ammonium perchlorate at 298 K is -295.31 kJ.mol-1 .Write the equation that corresponds to this value.

Accepted Answer

½N₂(g)+ ½Cl_2</

Question 2

Calculate the change in molar entropy when 2.00 mol of ozone are compressed isothermally to one quarter of its original volume .
Treat ozone as an ideal gas.

Accepted Answer

A)  -23.1 kJ.mol-1  
B)  -10.0 kJ.mol-1  
C)  -1.39 kJ.mol-1  
D)  +10.0 kJ.mol-1  
E)  +23.1 kJ.mol-1  
A)  -23.1 kJ.mol-1  
B)  -10.0 kJ.mol-1  
C)  -1.39 kJ.mol-1  
D)  +10.0 kJ.mol-1  
E)  +23.1 kJ.mol-1

Question 3

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether, which boils at 309 K.

Accepted Answer

A)  +85 kJ.mol-1  
B)  +26 kJ.mol-1  
C)  +275 kJ.mol-1  
D)  -85 kJ.mol-1  
E)  +3.6 kJ.mol-1  
A)  +85 kJ.mol-1  
B)  +26 kJ.mol-1  
C)  +275 kJ.mol-1  
D)  -85 kJ.mol-1  
E)  +3.6 kJ.mol-1

Question 4

Which of the following is always true for a spontaneous process at constant temperature?

Accepted Answer

A) $\Delta$Ssystem + $\Delta$Ssurroundings = q/T B) $\Delta$S > 0 C) $\Delta$S = q/T D) $\Delta$Ssystem + $\Delta$Ssurroundings > 0 E) $\Delta$S < q/T A) $\Delta$Ssystem + $\Delta$Ssurroundings = q/T B) $\Delta$S > 0 C) $\Delta$S = q/T D) $\Delta$Ssystem + $\Delta$Ssurroundings > 0 E) $\Delta$S < q/T

Question 5

An isothermal change is one that occurs at a constant temperature.

Accepted Answer

A) True 
 B)False

Question 6

The molar entropy of Pb(s) at 298 K is equal to

Accepted Answer

A)  CP × 298. 
B)  zero. 
C)  the sum of the integral of CPdT/T from 0 K to 298 K. 
A)  CP × 298. 
B)  zero. 
C)  the sum of the integral of CPdT/T from 0 K to 298 K.

Question 7

The change in molar entropy for vaporization of all liquids is about the same.

Accepted Answer

A) True 
 B)False

Question 8

All entropies of fusion are positive.

Accepted Answer

A) True 
 B)False

Question 9

Calculate the change in internal energy when 2.50 kJ of energy is transferred as heat to 1.50 mol BF3 at 298 K and 1 atm at constant volume.

Accepted Answer

A)  +1.00 kJ 
B)  +2.50 kJ 
C)  -1.50 kJ 
D)  -2.50 kJ 
E)  +1.50 kJ 
A)  +1.00 kJ 
B)  +2.50 kJ 
C)  -1.50 kJ 
D)  -2.50 kJ 
E)  +1.50 kJ

Question 10

The dehydrogenation of cyclohexane,C6H12(l),to form benzene,C6H6(l),is not spontaneous.However, the hydrogenation of ethene to form ethane is spontaneous.Calculate the reaction free energy for the coupled reaction
C6H12(l)+ 3CH2=CH2(g)$\rightarrow$C6H6(l)+ CH3CH3(g)

Accepted Answer

-205 kJ·mo

Question 11

For the reaction 2NH3(g)$\rightarrow$  3H2(g)+ N2(g),KP = 1.47 *10-6 at 298 K.Estimate the temperature at which KP = 0.0100.

Accepted Answer

The answer of For the reaction 2NH3(g)$\rightarrow$  3H2(g)+ N2(g),KP...

Question 12

Calculate the standard entropy for the following reaction from standard molar entropies.
NH4ClO4(s)+ Al(s)$\rightarrow$NH4Cl(s)+ Al2O3(s)

Accepted Answer

-69.01 J.K^-

Question 13

If an isolated system contained +5 kJ of energy, after 100 years $\Delta$U =

Accepted Answer

A)  The answer is impossible to determine 
B)  Slightly less than +5 kJ. 
C)  +5 kJ. 
D)  0 kJ. 
E)  -5 kJ. 
A)  The answer is impossible to determine 
B)  Slightly less than +5 kJ. 
C)  +5 kJ. 
D)  0 kJ. 
E)  -5 kJ.

Question 14

A reaction known to release 2.00 kJ of heat takes place in a calorimeter containing 0.200 L of solution and the temperature rose by 4.46$\omicron $C .When 100 mL of nitric acid and 100 mL of sodium hydroxide were mixed in the same calorimeter,The temperature rose 2.01$\omicron $C.What is the heat output for the neutralization reaction?

Accepted Answer

A)  0.0186 k.J.($\omicron $
C) -1  
B)  0.448 k.J.($\omicron $
C) -1  
C)  0.816 k.J.($\omicron $
C) -1  
D)  17.9 k.J.($\omicron $
C) -1  
E)  0.901 k.J.($\omicron $
C) -1  
A)  0.0186 k.J.($\omicron $
C) -1  
B)  0.448 k.J.($\omicron $
C) -1  
C)  0.816 k.J.($\omicron $
C) -1  
D)  17.9 k.J.($\omicron $
C) -1  
E)  0.901 k.J.($\omicron $
C) -1

Question 15

A piece of equipment must be capable of containing water at temperatures well above its normal boiling point.If the piece of equipment withstands an internal pressure of no more than 10.0 atm,calculate the highest temperature at which the system can be safely operated.

Accepted Answer

The answer of A piece of equipment must be capable...

Question 16

Under what conditions (e.g.,constant P)are the following relations true?
(a)$\Delta$G = $\Delta$H -T$\Delta$S
(b)q = $\Delta$H

Accepted Answer

(a)constan

Question 17

Calculate the final temperature when 2.50 kJ of energy is transferred as heat to 1.50 mol N2 at 298 K and 1 atm at constant pressure.

Accepted Answer

A)  75S1U1P1$\circ$S1S1P0C 
B)  159S1U1P1$\circ$S1S1P0C 
C)  80S1U1P1$\circ$S1S1P0C 
D)  82S1U1P1$\circ$S1S1P0C 
E)  92S1U1P1$\circ$S1S1P0C 
A)  75S1U1P1$\circ$S1S1P0C 
B)  159S1U1P1$\circ$S1S1P0C 
C)  80S1U1P1$\circ$S1S1P0C 
D)  82S1U1P1$\circ$S1S1P0C 
E)  92S1U1P1$\circ$S1S1P0C

Question 18

The formation of solid calcium oxide from a gas of its ions is an exothermic process and is equal to the reverse of the lattice enthalpy.

Accepted Answer

A) True 
 B)False

Question 19

The standard reaction free energy for the oxidation of glucose is -2879 kJ·mol-1.What is the maximum nonexpansion work obtainable from 125 g glucose,C6H12O6(s)?

Accepted Answer

The answer of The standard reaction free energy for the...

Question 20

Predict the sign of the molar Gibbs free energy for the process H2O(s)$\rightarrow$H2O(l)At 1 atm and 1oC,0oC, And -oC,Respectively.

Accepted Answer

A)  +, 0, and - 
B)  -, 0, and + 
C)  +, +, and- 
D)  -, -, and + 
E)  +, 0, and + 
A)  +, 0, and - 
B)  -, 0, and + 
C)  +, +, and- 
D)  -, -, and + 
E)  +, 0, and +

The standard enthalpy of formation of ammonium perchlorate at 298 K is -295.31 kJ.mol^-¹.Write the equation that corresponds to this value.

Calculate the change in molar entropy when 2.00 mol of ozone are compressed isothermally to one quarter of its original volume . Treat ozone as an ideal gas.

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether, which boils at 309 K.

Which of the following is always true for a spontaneous process at constant temperature?

An isothermal change is one that occurs at a constant temperature.

The molar entropy of Pb(s) at 298 K is equal to

The change in molar entropy for vaporization of all liquids is about the same.

All entropies of fusion are positive.

Calculate the change in internal energy when 2.50 kJ of energy is transferred as heat to 1.50 mol BF₃ at 298 K and 1 atm at constant volume.

The dehydrogenation of cyclohexane,C₆H₁₂(l),to form benzene,C₆H₆(l),is not spontaneous.However, the hydrogenation of ethene to form ethane is spontaneous.Calculate the reaction free energy for the coupled reaction C₆H₁₂(l)+ 3CH₂=CH₂(g) $\rightarrow$ C₆H₆(l)+ CH₃CH₃(g)

For the reaction 2NH₃(g) $\rightarrow$ 3H₂(g)+ N₂(g),K_P = 1.47 *10^-⁶ at 298 K.Estimate the temperature at which K_P = 0.0100.

Calculate the standard entropy for the following reaction from standard molar entropies. NH₄ClO₄(s)+ Al(s) $\rightarrow$ NH₄Cl(s)+ Al₂O₃_(s)

If an isolated system contained +5 kJ of energy, after 100 years $\Delta$ U =

A piece of equipment must be capable of containing water at temperatures well above its normal boiling point.If the piece of equipment withstands an internal pressure of no more than 10.0 atm,calculate the highest temperature at which the system can be safely operated.

Under what conditions (e.g.,constant P)are the following relations true? (a) $\Delta$ G = $\Delta$ H -T $\Delta$ S (b)q = $\Delta$ H

Calculate the final temperature when 2.50 kJ of energy is transferred as heat to 1.50 mol N₂ at 298 K and 1 atm at constant pressure.

The formation of solid calcium oxide from a gas of its ions is an exothermic process and is equal to the reverse of the lattice enthalpy.

The standard reaction free energy for the oxidation of glucose is -2879 kJ·mol^-¹.What is the maximum nonexpansion work obtainable from 125 g glucose,C₆H₁₂O₆(s)?

Predict the sign of the molar Gibbs free energy for the process H₂O(s) $\rightarrow$ H₂O(l)At 1 atm and 1^oC,0^oC, And -^oC,Respectively.

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Exam 4: Thermodynamics

The standard enthalpy of formation of ammonium perchlorate at 298 K is -295.31 kJ.mol-1 .Write the equation that corresponds to this value.

Calculate the change in molar entropy when 2.00 mol of ozone are compressed isothermally to one quarter of its original volume . Treat ozone as an ideal gas.

Use Trouton's constant to estimate the enthalpy of vaporization of diethyl ether, which boils at 309 K.

Which of the following is always true for a spontaneous process at constant temperature?

An isothermal change is one that occurs at a constant temperature.

The molar entropy of Pb(s) at 298 K is equal to

The change in molar entropy for vaporization of all liquids is about the same.

All entropies of fusion are positive.

Calculate the change in internal energy when 2.50 kJ of energy is transferred as heat to 1.50 mol BF3 at 298 K and 1 atm at constant volume.

The dehydrogenation of cyclohexane,C6H12(l),to form benzene,C6H6(l),is not spontaneous.However, the hydrogenation of ethene to form ethane is spontaneous.Calculate the reaction free energy for the coupled reaction C6H12(l)+ 3CH2=CH2(g) →\rightarrow→ C6H6(l)+ CH3CH3(g)

For the reaction 2NH3(g) →\rightarrow→ 3H2(g)+ N2(g),KP = 1.47 *10-6 at 298 K.Estimate the temperature at which KP = 0.0100.

Calculate the standard entropy for the following reaction from standard molar entropies. NH4ClO4(s)+ Al(s) →\rightarrow→ NH4Cl(s)+ Al2O3(s)

If an isolated system contained +5 kJ of energy, after 100 years Δ\DeltaΔ U =

A piece of equipment must be capable of containing water at temperatures well above its normal boiling point.If the piece of equipment withstands an internal pressure of no more than 10.0 atm,calculate the highest temperature at which the system can be safely operated.

Under what conditions (e.g.,constant P)are the following relations true? (a) Δ\DeltaΔ G = Δ\DeltaΔ H -T Δ\DeltaΔ S (b)q = Δ\DeltaΔ H

Calculate the final temperature when 2.50 kJ of energy is transferred as heat to 1.50 mol N2 at 298 K and 1 atm at constant pressure.

The formation of solid calcium oxide from a gas of its ions is an exothermic process and is equal to the reverse of the lattice enthalpy.

The standard reaction free energy for the oxidation of glucose is -2879 kJ·mol-1.What is the maximum nonexpansion work obtainable from 125 g glucose,C6H12O6(s)?

Predict the sign of the molar Gibbs free energy for the process H2O(s) →\rightarrow→ H2O(l)At 1 atm and 1oC,0oC, And -oC,Respectively.

Atoms

Molecules

States of Matter

Equilibrium

Reactions

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

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The standard enthalpy of formation of ammonium perchlorate at 298 K is -295.31 kJ.mol^-¹.Write the equation that corresponds to this value.

Calculate the change in internal energy when 2.50 kJ of energy is transferred as heat to 1.50 mol BF₃ at 298 K and 1 atm at constant volume.

The dehydrogenation of cyclohexane,C₆H₁₂(l),to form benzene,C₆H₆(l),is not spontaneous.However, the hydrogenation of ethene to form ethane is spontaneous.Calculate the reaction free energy for the coupled reaction C₆H₁₂(l)+ 3CH₂=CH₂(g) $\rightarrow$ C₆H₆(l)+ CH₃CH₃(g)

For the reaction 2NH₃(g) $\rightarrow$ 3H₂(g)+ N₂(g),K_P = 1.47 *10^-⁶ at 298 K.Estimate the temperature at which K_P = 0.0100.

Calculate the standard entropy for the following reaction from standard molar entropies. NH₄ClO₄(s)+ Al(s) $\rightarrow$ NH₄Cl(s)+ Al₂O₃_(s)

If an isolated system contained +5 kJ of energy, after 100 years $\Delta$ U =

Under what conditions (e.g.,constant P)are the following relations true? (a) $\Delta$ G = $\Delta$ H -T $\Delta$ S (b)q = $\Delta$ H

Calculate the final temperature when 2.50 kJ of energy is transferred as heat to 1.50 mol N₂ at 298 K and 1 atm at constant pressure.

The standard reaction free energy for the oxidation of glucose is -2879 kJ·mol^-¹.What is the maximum nonexpansion work obtainable from 125 g glucose,C₆H₁₂O₆(s)?

Predict the sign of the molar Gibbs free energy for the process H₂O(s) $\rightarrow$ H₂O(l)At 1 atm and 1^oC,0^oC, And -^oC,Respectively.