Question 1

The solubility of oxygen at a certain temperature is 8 ppm.If the partial pressure of oxygen is doubled at this temperature,the solubility is 16 ppm.

Accepted Answer

A) True 
 B)False

Question 2

Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the following observations: A thin wire with weights attached is draped over a block of "dry ice," a second wire with weights is draped over a block of ice.The wire cuts through the ice but not through the "dry ice."

Accepted Answer

For water,increased pressure r

Question 3

The reaction free energy $\Delta$Gr = $\Delta$G°r F1F1F1S1-F1F1F10 RTln(K).

Accepted Answer

A) True 
 B)False

Question 4

The equilibrium constant for the reaction
HNO2(aq)+ H2O(l)F1S1S1W1$\rightarrow$F1F1F10NO2F1F1F1S1-F1F1F10(aq)+ H3O+(aq)
is 4.3 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F104 at 25$\omicron$C.Will nitrous acid spontaneously dissociate when
[HNO2(aq)] = 1.0 M and [NO2F1F1F1S1-F1F1F10(aq)] = [H3O+(aq)] = 1.0 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F105 M?
Show your calculations.

Accepted Answer

Question 5

Consider the following
N2O4(g)
 $f$ 
2NO2(g)
The equilibrium constant for this reaction will decrease with an increase in temperature.

Accepted Answer

A) True 
 B)False

Question 6

The phase diagram for a pure substance is shown below.   What is the lowest temperature at which liquid can exist?

Accepted Answer

A)  400 K 
B)  0 K 
C)  200 K 
D)  150 K 
E)  250 K 
A)  400 K 
B)  0 K 
C)  200 K 
D)  150 K 
E)  250 K

Question 7

Consider the reaction
2CuBr2(s)$\rightarrow$2CuBr(s)+ Br2(g)If the equilibrium vapor pressure of Br2(g)
Is 1.43 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F105 Torr at 298 K,What is $\Delta$G at this temperature when Br2(g)
Is produced at a pressure of 7.50 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F107 Torr?

Accepted Answer

A)  F1F1F1S1-F1F1F107.31 kJ 
B)  7.31 kJ 
C)  39.9 kJ 
D)  F1F1F1S1-F1F1F103.17 kJ 
E)  F1F1F1S1-F1F1F104.15 kJ 
A)  F1F1F1S1-F1F1F107.31 kJ 
B)  7.31 kJ 
C)  39.9 kJ 
D)  F1F1F1S1-F1F1F103.17 kJ 
E)  F1F1F1S1-F1F1F104.15 kJ

Question 8

Given: C(s) + CO2(g) $f$
2CO(g)
At equilibrium at a certain temperature,The partial pressures of CO(g)
And CO2(g)Are 1.22 atm and 0.780 atm,Respectively.Calculate the value of K for this reaction.

Accepted Answer

A)  3.13 
B)  2.00 
C)  1.91 
D)  1.56 
E)  0.640 
A)  3.13 
B)  2.00 
C)  1.91 
D)  1.56 
E)  0.640

Question 9

Estimate the enthalpy of vaporization of water given that at 25$\omicron$C and 35F$\omicron$C its vapor pressure is 23.8 and 42 Torr, respectively.Assume that the enthalpy of vaporization is independent of the temperature.

Accepted Answer

A)  415 JF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
B)  221 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
C)  41.5 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
D)  5.21 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
E)  43.4 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
A)  415 JF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
B)  221 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
C)  41.5 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
D)  5.21 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
E)  43.4 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101

Question 10

For the reaction 2NOCl(g) $f$ 
2NO(g)+ Cl2(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl2(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Accepted Answer

Question 11

A mixture consisting of 0.250 M N2(g) and 0.500 M H2(g)
Reaches equilibrium according to the equation below:
N2(g)3H2(g) $f$
2NH3(g)
At equilibrium,
The concentration of ammonia is 0.150 M.Calculate the concentration of N2(g)At equilibrium.

Accepted Answer

A)  0.150 M 
B)  0.100 M 
C)  0.0750 M 
D)  0.0500 M 
E)  0.175 M 
A)  0.150 M 
B)  0.100 M 
C)  0.0750 M 
D)  0.0500 M 
E)  0.175 M

Question 12

The phase diagram for sulfur is given below.   The number of phases that sulfur can exist in and the number of triple points,Respectively,Are

Accepted Answer

A)  3 and 2. 
B)  3 and 3. 
C)  4 and 2. 
D)  3 and 1. 
E)  4 and 3. 
A)  3 and 2. 
B)  3 and 3. 
C)  4 and 2. 
D)  3 and 1. 
E)  4 and 3.

Question 13

Consider the reaction
PCl5(g) $f$
PCl3(g)+ Cl2(g)
At a certain temperature,If the initial concentration of PCl5(g)Is 3.0 M,At equilibrium the concentration of Cl2(g)Is 0.80 M.Calculate the value of Kc at this temperature.

Accepted Answer

A)  0.21 
B)  0.29 
C)  0.64 
D)  3.4 
E)  0.46 
A)  0.21 
B)  0.29 
C)  0.64 
D)  3.4 
E)  0.46

Question 14

For AlF3,the lattice enthalpy is 5220 kJ.mol-1  and the enthalpy of solution is F1F1F1S1-F1F1F1027 kJ.mol-1  at 25$\omicron$C.Calculate the enthalpy of hydration of AlF3 at this temperature.

Accepted Answer

F1F1F1S1?F1F1F105247

Question 15

Consider the diagram below.    
(a)What is the mixture in the diagram called?
(b)Can the components of this mixture be separated by fractional distillation? Explain.

Accepted Answer

(a)Minimum-boiling azeotrope
(

Question 16

Calculate$\Delta$G at 298 K for the reaction
C2H5OH(l)$\rightarrow$C2H5OH(g,0.0263 bar)
Given $\Delta$G$\omicron$ = 6.2 kJ at 298 K.

Accepted Answer

A)  6.2 kJ 
B)  15 kJ 
C)  2.8 kJ 
D)  -2.8 kJ 
E)  -15 kJ 
A)  6.2 kJ 
B)  15 kJ 
C)  2.8 kJ 
D)  -2.8 kJ 
E)  -15 kJ

Question 17

Consider the following reaction at a certain temperature:
Ni(s)+ 4CO(g)$f$ Ni(CO)4(g)Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)4(g) are 1.25 and 6.65 atm over 1.00 kg of nickel.

Accepted Answer

Question 18

For the reaction Br2(g)
 $f$ 
2Br(g),F1F1F1S1?F1F1F10Gro = +161.69 kJ·molF1F1F1S1-F1F1F101 at 25F1F1F1S1?F1F1F10C.Calculate the value of Kc for this reaction.

Accepted Answer

A)  0.0378 
B)  1.12 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1027 
C)  1.83 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1030 
D)  4.54 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1029 
A)  0.0378 
B)  1.12 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1027 
C)  1.83 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1030 
D)  4.54 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1029

Question 19

At 600F1F1F1S1?F1F1F10C, the equilibrium constant for the reaction
2HgO(s) $f$
2Hg(l)+ O2(g)
Is 2.8.Calculate the equilibrium constant for the reaction $\frac { 1 } { 2 }$
1/2O2(g)+ Hg(l) 
$f$
HgO(s)

Accepted Answer

A)  F1F1F1S1-F1F1F101.7 
B)  1.1 
C)  0.60 
D)  0.36 
E)  1.7 
A)  F1F1F1S1-F1F1F101.7 
B)  1.1 
C)  0.60 
D)  0.36 
E)  1.7

Question 20

The phase diagram for a pure substance is given below .What is the critical temperature?

Accepted Answer

A)  0 K 
B)  250 K 
C)  300 K 
D)  400 K 
E)  200 K 
A)  0 K 
B)  250 K 
C)  300 K 
D)  400 K 
E)  200 K

The solubility of oxygen at a certain temperature is 8 ppm.If the partial pressure of oxygen is doubled at this temperature,the solubility is 16 ppm.

The reaction free energy $\Delta$ G_r = $\Delta$ G°_r - RTln(K).

The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) $\rightarrow$ NO₂-(aq)+ H₃O⁺(aq) is 4.3 * 10^-⁴ at 25^$\omicron$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-⁵ M? Show your calculations.

Consider the following N₂O₄(g) $f$ 2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

The phase diagram for a pure substance is shown below. What is the lowest temperature at which liquid can exist?

Consider the reaction 2CuBr₂(s) $\rightarrow$ 2CuBr(s)+ Br₂(g)If the equilibrium vapor pressure of Br₂(g) Is 1.43 * 10^-⁵ Torr at 298 K,What is $\Delta$ G at this temperature when Br₂(g) Is produced at a pressure of 7.50 * 10^-⁷ Torr?

Given: C(s) + CO₂(g) $f$ 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g) And CO₂(g)Are 1.22 atm and 0.780 atm,Respectively.Calculate the value of K for this reaction.

Estimate the enthalpy of vaporization of water given that at 25^$\omicron$C and 35F^$\omicron$C its vapor pressure is 23.8 and 42 Torr, respectively.Assume that the enthalpy of vaporization is independent of the temperature.

For the reaction 2NOCl(g) $f$ 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

A mixture consisting of 0.250 M N₂(g) and 0.500 M H₂(g) Reaches equilibrium according to the equation below: N₂(g)3H₂(g) $f$ 2NH₃(g) At equilibrium, The concentration of ammonia is 0.150 M.Calculate the concentration of N₂(g)At equilibrium.

The phase diagram for sulfur is given below. The number of phases that sulfur can exist in and the number of triple points,Respectively,Are

Consider the reaction PCl₅(g) $f$ PCl₃(g)+ Cl₂(g) At a certain temperature,If the initial concentration of PCl₅(g)Is 3.0 M,At equilibrium the concentration of Cl₂(g)Is 0.80 M.Calculate the value of K_c at this temperature.

For AlF₃,the lattice enthalpy is 5220 kJ.mol^-¹ and the enthalpy of solution is -27 kJ.mol^-¹ at 25^$\omicron$C.Calculate the enthalpy of hydration of AlF₃ at this temperature.

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0263 bar) Given $\Delta$ G^$\omicron$= 6.2 kJ at 298 K.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) $f$ Ni(CO)₄(g)Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g) are 1.25 and 6.65 atm over 1.00 kg of nickel.

For the reaction Br₂(g) $f$ 2Br(g),?G_r^o = +161.69 kJ·mol^-¹ at 25?C.Calculate the value of K_c for this reaction.

At 600?C, the equilibrium constant for the reaction 2HgO(s) $f$ 2Hg(l)+ O₂(g) Is 2.8.Calculate the equilibrium constant for the reaction $\frac { 1 } { 2 }$ 1/2O₂(g)+ Hg(l) $f$ HgO(s)

The phase diagram for a pure substance is given below .What is the critical temperature?

Atoms

Molecules

States of Matter

Thermodynamics

Reactions

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Exam 5: Equilibrium

The solubility of oxygen at a certain temperature is 8 ppm.If the partial pressure of oxygen is doubled at this temperature,the solubility is 16 ppm.

The reaction free energy Δ\DeltaΔ Gr = Δ\DeltaΔ G°r - RTln(K).

The equilibrium constant for the reaction HNO2(aq)+ H2O(l) →\rightarrow→ NO2-(aq)+ H3O+(aq) is 4.3 * 10-4 at 25 ο\omicronο C.Will nitrous acid spontaneously dissociate when [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0 * 10-5 M? Show your calculations.

Consider the following N2O4(g) fff 2NO2(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

The phase diagram for a pure substance is shown below. What is the lowest temperature at which liquid can exist?

Consider the reaction 2CuBr2(s) →\rightarrow→ 2CuBr(s)+ Br2(g)If the equilibrium vapor pressure of Br2(g) Is 1.43 * 10-5 Torr at 298 K,What is Δ\DeltaΔ G at this temperature when Br2(g) Is produced at a pressure of 7.50 * 10-7 Torr?

Given: C(s) + CO2(g) fff 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g) And CO2(g)Are 1.22 atm and 0.780 atm,Respectively.Calculate the value of K for this reaction.

Estimate the enthalpy of vaporization of water given that at 25 ο\omicronο C and 35F ο\omicronο C its vapor pressure is 23.8 and 42 Torr, respectively.Assume that the enthalpy of vaporization is independent of the temperature.

For the reaction 2NOCl(g) fff 2NO(g)+ Cl2(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl2(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

A mixture consisting of 0.250 M N2(g) and 0.500 M H2(g) Reaches equilibrium according to the equation below: N2(g)3H2(g) fff 2NH3(g) At equilibrium, The concentration of ammonia is 0.150 M.Calculate the concentration of N2(g)At equilibrium.

The phase diagram for sulfur is given below. The number of phases that sulfur can exist in and the number of triple points,Respectively,Are

Consider the reaction PCl5(g) fff PCl3(g)+ Cl2(g) At a certain temperature,If the initial concentration of PCl5(g)Is 3.0 M,At equilibrium the concentration of Cl2(g)Is 0.80 M.Calculate the value of Kc at this temperature.

For AlF3,the lattice enthalpy is 5220 kJ.mol-1 and the enthalpy of solution is -27 kJ.mol-1 at 25 ο\omicronο C.Calculate the enthalpy of hydration of AlF3 at this temperature.

Consider the diagram below. (a)What is the mixture in the diagram called? (b)Can the components of this mixture be separated by fractional distillation? Explain.

Calculate Δ\DeltaΔ G at 298 K for the reaction C2H5OH(l) →\rightarrow→ C2H5OH(g,0.0263 bar) Given Δ\DeltaΔ G ο\omicronο = 6.2 kJ at 298 K.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) fff Ni(CO)4(g)Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)4(g) are 1.25 and 6.65 atm over 1.00 kg of nickel.

For the reaction Br2(g) fff 2Br(g),?Gro = +161.69 kJ·mol-1 at 25?C.Calculate the value of Kc for this reaction.

At 600?C, the equilibrium constant for the reaction 2HgO(s) fff 2Hg(l)+ O2(g) Is 2.8.Calculate the equilibrium constant for the reaction 12\frac { 1 } { 2 }21​ 1/2O2(g)+ Hg(l) fff HgO(s)

The phase diagram for a pure substance is given below .What is the critical temperature?

Atoms

Molecules

States of Matter

Thermodynamics

Reactions

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

The reaction free energy $\Delta$ G_r = $\Delta$ G°_r - RTln(K).

The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) $\rightarrow$ NO₂-(aq)+ H₃O⁺(aq) is 4.3 * 10^-⁴ at 25^$\omicron$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-⁵ M? Show your calculations.

Consider the following N₂O₄(g) $f$ 2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction 2CuBr₂(s) $\rightarrow$ 2CuBr(s)+ Br₂(g)If the equilibrium vapor pressure of Br₂(g) Is 1.43 * 10^-⁵ Torr at 298 K,What is $\Delta$ G at this temperature when Br₂(g) Is produced at a pressure of 7.50 * 10^-⁷ Torr?

Given: C(s) + CO₂(g) $f$ 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g) And CO₂(g)Are 1.22 atm and 0.780 atm,Respectively.Calculate the value of K for this reaction.

Estimate the enthalpy of vaporization of water given that at 25^$\omicron$C and 35F^$\omicron$C its vapor pressure is 23.8 and 42 Torr, respectively.Assume that the enthalpy of vaporization is independent of the temperature.

For the reaction 2NOCl(g) $f$ 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

A mixture consisting of 0.250 M N₂(g) and 0.500 M H₂(g) Reaches equilibrium according to the equation below: N₂(g)3H₂(g) $f$ 2NH₃(g) At equilibrium, The concentration of ammonia is 0.150 M.Calculate the concentration of N₂(g)At equilibrium.

Consider the reaction PCl₅(g) $f$ PCl₃(g)+ Cl₂(g) At a certain temperature,If the initial concentration of PCl₅(g)Is 3.0 M,At equilibrium the concentration of Cl₂(g)Is 0.80 M.Calculate the value of K_c at this temperature.

For AlF₃,the lattice enthalpy is 5220 kJ.mol^-¹ and the enthalpy of solution is -27 kJ.mol^-¹ at 25^$\omicron$C.Calculate the enthalpy of hydration of AlF₃ at this temperature.

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0263 bar) Given $\Delta$ G^$\omicron$= 6.2 kJ at 298 K.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) $f$ Ni(CO)₄(g)Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g) are 1.25 and 6.65 atm over 1.00 kg of nickel.

For the reaction Br₂(g) $f$ 2Br(g),?G_r^o = +161.69 kJ·mol^-¹ at 25?C.Calculate the value of K_c for this reaction.

At 600?C, the equilibrium constant for the reaction 2HgO(s) $f$ 2Hg(l)+ O₂(g) Is 2.8.Calculate the equilibrium constant for the reaction $\frac { 1 } { 2 }$ 1/2O₂(g)+ Hg(l) $f$ HgO(s)