Question 1

Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

Accepted Answer

A) True 
 B)False

Question 2

The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr, respectively,At 296 K.What is the vapor pressure of a solution containing 50.0 g of each compound?

Accepted Answer

A)  260 Torr 
B)  274 Torr 
C)  241 Torr 
D)  33.0 Torr 
E)  460 Torr 
A)  260 Torr 
B)  274 Torr 
C)  241 Torr 
D)  33.0 Torr 
E)  460 Torr

Question 3

The vapor pressure of water at 37$\omicron$C is 47.1 Torr and its enthalpy of vaporization is 44.0 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 .Estimate the vapor pressure of water at 87$\omicron$C.Assume that the enthalpy of vaporization of water is independent of temperature.

Accepted Answer

A)  112 Torr 
B)  256 Torr 
C)  713 Torr 
D)  52 Torr 
E)  504 Torr 
A)  112 Torr 
B)  256 Torr 
C)  713 Torr 
D)  52 Torr 
E)  504 Torr

Question 4

The enthalpy of hydration of AgBr is F1F1F1S1-F1F1F10819 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 at 25$\omicron$C .Given that the hydration enthalpy of BrF1F1F1S1-F1F1F10 is F1F1F1S1-F1F1F10309 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101,Calculate the enthalpy of hydration of Ag+ ions.

Accepted Answer

A)  F1F1F1S1-F1F1F10410 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
B)  F1F1F1S1-F1F1F10819 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
C)  F1F1F1S1-F1F1F101128 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
D)  F1F1F1S1-F1F1F10309 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
E)  F1F1F1S1-F1F1F10510 kJF1F1F1S1?F1F1F10molF1F1F1S1?F1F1F101  
A)  F1F1F1S1-F1F1F10410 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
B)  F1F1F1S1-F1F1F10819 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
C)  F1F1F1S1-F1F1F101128 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
D)  F1F1F1S1-F1F1F10309 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101 
E)  F1F1F1S1-F1F1F10510 kJF1F1F1S1?F1F1F10molF1F1F1S1?F1F1F101

Question 5

Calculate the molality of perchloric acid in 9.2 M HClO4(aq).The density of this solution is 1.54 g/mL.

Accepted Answer

Question 6

Which of the following statements is true regarding solubility? Assume that the solute does not affect the solvent and we are dealing with dilute solutions.

Accepted Answer

A)  We can expect substances with positive enthalpies of solution always to be soluble. 
B)  We can expect substances with positive enthalpies of solution always to be soluble only if the entropy of solution is negative. 
C)  All the other statements are false because the solute always affects the solvent resulting in a negative entropy of solution. 
D)  We can expect substances with negative enthalpies of solution always to be soluble. 
E)  We can expect substances with positive enthalpies of solution always to be soluble only if the entropy of solution is positive. 
A)  We can expect substances with positive enthalpies of solution always to be soluble. 
B)  We can expect substances with positive enthalpies of solution always to be soluble only if the entropy of solution is negative. 
C)  All the other statements are false because the solute always affects the solvent resulting in a negative entropy of solution. 
D)  We can expect substances with negative enthalpies of solution always to be soluble. 
E)  We can expect substances with positive enthalpies of solution always to be soluble only if the entropy of solution is positive.

Question 7

Given: C(s) + CO2(g) $f$
2CO(g)
At equilibrium at a certain temperature,The partial pressures of CO(g)And CO2(g)Are 1.44 atm and 0.820 atm,Respectively.Calculate the value of K for this reaction.

Accepted Answer

A)  2.53 
B)  10.1 
C)  1.76 
D)  3.08 
E)  3.51 
A)  2.53 
B)  10.1 
C)  1.76 
D)  3.08 
E)  3.51

Question 8

The addition of 125 mg of caffeine to 100 g of cyclohexane lowered the freezing point by 0.13 K .Calculate the molar mass of caffeine.The kf for cyclohexane is 20.1 KF1F1F1S1.F1F1F10kgF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101.

Accepted Answer

A)  47.8 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
B)  481 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
C)  96.5 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
D)  19.3 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
E)  193 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
A)  47.8 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
B)  481 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
C)  96.5 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
D)  19.3 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101  
E)  193 gF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101

Question 9

Consider the reaction
4NH3(g)+ 7O2(g) 
$f$ 
2N2O4(g)+ 6H2O(g)If,initially,[NH3(g)] = [O2(g)] = 3.60 M,at equilibrium,[N2O4(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

Accepted Answer

[NH₃(g)] = 2.40 M, [O

Question 10

A plot of ln(vapor pressure) versus 1/T for benzene gives a straight line with slope F1F1F1S1-F1F1F103.70 F1F1F1S1*F1F1F10 103 K.The enthalpy of vaporization of benzene is

Accepted Answer

A)  2.25 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
B)  Not enough information is given to permit the calculation. 
C)  3.70 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
D)  30.8 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
E)  445 JF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
A)  2.25 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
B)  Not enough information is given to permit the calculation. 
C)  3.70 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
D)  30.8 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
E)  445 JF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101.

Question 11

The equilibrium constant, Kc,For the reaction
2NOCl(g) $f$
2NO(g)+ Cl2(g)
Is 0.51 at a certain temperature.A mixture of NOCl,
NO,And Cl2 with concentrations1.3,1.2,And 0.60 M,Respectively,
Was introduced into a container at this temperature.Which of the following is true?

Accepted Answer

A)  Cl2(g) is produced until equilibrium is reached. 
B)  [NOCl] = [NO] = [Cl2] at equilibrium. 
C)  NOCl(g) is produced until equilibrium is reached. 
D)  [Cl2] = 0.30 M at equilibrium. 
E)  No apparent reaction takes place. 
A)  Cl2(g) is produced until equilibrium is reached. 
B)  [NOCl] = [NO] = [Cl2] at equilibrium. 
C)  NOCl(g) is produced until equilibrium is reached. 
D)  [Cl2] = 0.30 M at equilibrium. 
E)  No apparent reaction takes place.

Question 12

the boiling point of water is higher in a pressure cooker than the normal boiling point?

Accepted Answer

A) True 
 B)False

Question 13

Benzene would likely dissolve which of the following substances?

Accepted Answer

A)  Cl2CCCl2 
B)  NaCl  
C)  Na2CO3  
D)  Ca(HCO3)2  
E)  C6H12O6  
A)  Cl2CCCl2 
B)  NaCl  
C)  Na2CO3  
D)  Ca(HCO3)2  
E)  C6H12O6

Question 14

At 600F1F1F1S1?F1F1F10C, Kc = 2.8 for the reaction
2HgO(s)$f$2Hg(l)+ O2(g)
Calculate K at 600F1F1F1S1?F1F1F10C for this reaction.

Accepted Answer

A)  6800 
B)  200 
C)  1.4 F1F1F1S1*F1F1F10 104  
D)  2.8 
E)  138 
A)  6800 
B)  200 
C)  1.4 F1F1F1S1*F1F1F10 104  
D)  2.8 
E)  138

Question 15

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

Accepted Answer

A) True 
 B)False

Question 16

The vapor pressure of acetic acid at 25F1F1F1S1?F1F1F10C is 16 Torr . F1F1F1S1?F1F1F10Gr for the reaction
CH3COOH(l) $f$
CH3COOH(g)
At 25F1F1F1S1?F1F1F10C is

Accepted Answer

A)  0 
B)  +9.57 kJ·molF1F1F1S1-F1F1F101 
C)  F1F1F1S1-F1F1F109.57 kJ·molF1F1F1S1-F1F1F101 
D)  +1.85 kJ·molF1F1F1S1-F1F1F101 
A)  0 
B)  +9.57 kJ·molF1F1F1S1-F1F1F101 
C)  F1F1F1S1-F1F1F109.57 kJ·molF1F1F1S1-F1F1F101 
D)  +1.85 kJ·molF1F1F1S1-F1F1F101

Question 17

What is the relation between K and Kc for the reaction
H2(g)+ I2(g)F1S1S1W1?F1F1F102HI(g)

Accepted Answer

A)  K = Kc  
B)  K = RTKc  
C)  Kc = (RT)2K 
D)  K = (RT)2Kc  
E)  Kc = RTK 
A)  K = Kc  
B)  K = RTKc  
C)  Kc = (RT)2K 
D)  K = (RT)2Kc  
E)  Kc = RTK

Question 18

Which of the following statements is true?

Accepted Answer

A)  When the value of Q is large, the equilibrium lies on the product side of the equilibrium reaction. 
B)  When the value of K is large, the equilibrium lies on the reactant side of the equilibrium reaction. 
C)  A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products. 
D)  A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. 
E)  When the value of K is small, the equilibrium lies on the product side of the equilibrium reaction. 
A)  When the value of Q is large, the equilibrium lies on the product side of the equilibrium reaction. 
B)  When the value of K is large, the equilibrium lies on the reactant side of the equilibrium reaction. 
C)  A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products. 
D)  A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. 
E)  When the value of K is small, the equilibrium lies on the product side of the equilibrium reaction.

Question 19

Which of the following is likely to have the smallest exothermic hydration enthalpy?

Accepted Answer

A)  FF1F1F1S1F1F1F10  
B)  IF1F1F1S1F1F1F10  
C)  NO3F1F1F1S1F1F1F10  
D)  ClF1F1F1S1F1F1F10  
E)  BrF1F1F1S1F1F1F10  
A)  FF1F1F1S1F1F1F10  
B)  IF1F1F1S1F1F1F10  
C)  NO3F1F1F1S1F1F1F10  
D)  ClF1F1F1S1F1F1F10  
E)  BrF1F1F1S1F1F1F10

Question 20

Given:
4NH3(g)+ 5O2(g) $f$
4NO(g)+ 6H2O(g)
K
Calculate the equilibrium constant for the following reaction.
2NH3(g)+ $\frac { 5 } { 2 }$O2(g) $f$
2NO(g)+ 3H2O(g)

Accepted Answer

A)  K 
B)  KF1F1F1S1-F1F1F101  
C)  2K 
D)  0.5K 
E)  K1/2  
A)  K 
B)  KF1F1F1S1-F1F1F101  
C)  2K 
D)  0.5K 
E)  K1/2

Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr, respectively,At 296 K.What is the vapor pressure of a solution containing 50.0 g of each compound?

The vapor pressure of water at 37^$\omicron$C is 47.1 Torr and its enthalpy of vaporization is 44.0 kJ.mol^-¹ .Estimate the vapor pressure of water at 87^$\omicron$C.Assume that the enthalpy of vaporization of water is independent of temperature.

The enthalpy of hydration of AgBr is -819 kJ.mol^-¹ at 25^$\omicron$C .Given that the hydration enthalpy of Br^- is -309 kJ.mol^-¹,Calculate the enthalpy of hydration of Ag⁺ ions.

Calculate the molality of perchloric acid in 9.2 M HClO₄(aq).The density of this solution is 1.54 g/mL.

Which of the following statements is true regarding solubility? Assume that the solute does not affect the solvent and we are dealing with dilute solutions.

Given: C(s) + CO₂(g) $f$ 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g)And CO₂(g)Are 1.44 atm and 0.820 atm,Respectively.Calculate the value of K for this reaction.

The addition of 125 mg of caffeine to 100 g of cyclohexane lowered the freezing point by 0.13 K .Calculate the molar mass of caffeine.The k_f for cyclohexane is 20.1 K.kg.mol^-¹.

Consider the reaction 4NH₃(g)+ 7O₂(g) $f$ 2N₂O₄(g)+ 6H₂O(g)If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

A plot of ln(vapor pressure) versus 1/T for benzene gives a straight line with slope -3.70 * 10³ K.The enthalpy of vaporization of benzene is

The equilibrium constant, K_c,For the reaction 2NOCl(g) $f$ 2NO(g)+ Cl₂(g) Is 0.51 at a certain temperature.A mixture of NOCl, NO,And Cl₂ with concentrations1.3,1.2,And 0.60 M,Respectively, Was introduced into a container at this temperature.Which of the following is true?

the boiling point of water is higher in a pressure cooker than the normal boiling point?

Benzene would likely dissolve which of the following substances?

At 600?C, K_c = 2.8 for the reaction 2HgO(s) $f$ 2Hg(l)+ O₂(g) Calculate K at 600?C for this reaction.

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

The vapor pressure of acetic acid at 25?C is 16 Torr . ?G_r for the reaction CH₃COOH(l) $f$ CH₃COOH(g) At 25?C is

What is the relation between K and K_c for the reaction H₂(g)+ I₂(g)?2HI(g)

Which of the following statements is true?

Which of the following is likely to have the smallest exothermic hydration enthalpy?

Given: 4NH₃(g)+ 5O₂(g) $f$ 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NH₃(g)+ $\frac { 5 } { 2 }$ O₂(g) $f$ 2NO(g)+ 3H₂O(g)

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Exam 5: Equilibrium

Consider the phase diagram for sulfur in the text on page 316.Monoclinic sulfur is denser than rhombic sulfur.

The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr, respectively,At 296 K.What is the vapor pressure of a solution containing 50.0 g of each compound?

The vapor pressure of water at 37 ο\omicronο C is 47.1 Torr and its enthalpy of vaporization is 44.0 kJ.mol-1 .Estimate the vapor pressure of water at 87 ο\omicronο C.Assume that the enthalpy of vaporization of water is independent of temperature.

The enthalpy of hydration of AgBr is -819 kJ.mol-1 at 25 ο\omicronο C .Given that the hydration enthalpy of Br- is -309 kJ.mol-1,Calculate the enthalpy of hydration of Ag+ ions.

Calculate the molality of perchloric acid in 9.2 M HClO4(aq).The density of this solution is 1.54 g/mL.

Which of the following statements is true regarding solubility? Assume that the solute does not affect the solvent and we are dealing with dilute solutions.

Given: C(s) + CO2(g) fff 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g)And CO2(g)Are 1.44 atm and 0.820 atm,Respectively.Calculate the value of K for this reaction.

The addition of 125 mg of caffeine to 100 g of cyclohexane lowered the freezing point by 0.13 K .Calculate the molar mass of caffeine.The kf for cyclohexane is 20.1 K.kg.mol-1.

Consider the reaction 4NH3(g)+ 7O2(g) fff 2N2O4(g)+ 6H2O(g)If,initially,[NH3(g)] = [O2(g)] = 3.60 M,at equilibrium,[N2O4(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

A plot of ln(vapor pressure) versus 1/T for benzene gives a straight line with slope -3.70 * 103 K.The enthalpy of vaporization of benzene is

The equilibrium constant, Kc,For the reaction 2NOCl(g) fff 2NO(g)+ Cl2(g) Is 0.51 at a certain temperature.A mixture of NOCl, NO,And Cl2 with concentrations1.3,1.2,And 0.60 M,Respectively, Was introduced into a container at this temperature.Which of the following is true?

the boiling point of water is higher in a pressure cooker than the normal boiling point?

Benzene would likely dissolve which of the following substances?

At 600?C, Kc = 2.8 for the reaction 2HgO(s) fff 2Hg(l)+ O2(g) Calculate K at 600?C for this reaction.

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

The vapor pressure of acetic acid at 25?C is 16 Torr . ?Gr for the reaction CH3COOH(l) fff CH3COOH(g) At 25?C is

What is the relation between K and Kc for the reaction H2(g)+ I2(g)?2HI(g)

Which of the following statements is true?

Which of the following is likely to have the smallest exothermic hydration enthalpy?

Given: 4NH3(g)+ 5O2(g) fff 4NO(g)+ 6H2O(g) K Calculate the equilibrium constant for the following reaction. 2NH3(g)+ 52\frac { 5 } { 2 }25​ O2(g) fff 2NO(g)+ 3H2O(g)

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The vapor pressure of water at 37^$\omicron$C is 47.1 Torr and its enthalpy of vaporization is 44.0 kJ.mol^-¹ .Estimate the vapor pressure of water at 87^$\omicron$C.Assume that the enthalpy of vaporization of water is independent of temperature.

The enthalpy of hydration of AgBr is -819 kJ.mol^-¹ at 25^$\omicron$C .Given that the hydration enthalpy of Br^- is -309 kJ.mol^-¹,Calculate the enthalpy of hydration of Ag⁺ ions.

Calculate the molality of perchloric acid in 9.2 M HClO₄(aq).The density of this solution is 1.54 g/mL.

Given: C(s) + CO₂(g) $f$ 2CO(g) At equilibrium at a certain temperature,The partial pressures of CO(g)And CO₂(g)Are 1.44 atm and 0.820 atm,Respectively.Calculate the value of K for this reaction.

The addition of 125 mg of caffeine to 100 g of cyclohexane lowered the freezing point by 0.13 K .Calculate the molar mass of caffeine.The k_f for cyclohexane is 20.1 K.kg.mol^-¹.

Consider the reaction 4NH₃(g)+ 7O₂(g) $f$ 2N₂O₄(g)+ 6H₂O(g)If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

A plot of ln(vapor pressure) versus 1/T for benzene gives a straight line with slope -3.70 * 10³ K.The enthalpy of vaporization of benzene is

The equilibrium constant, K_c,For the reaction 2NOCl(g) $f$ 2NO(g)+ Cl₂(g) Is 0.51 at a certain temperature.A mixture of NOCl, NO,And Cl₂ with concentrations1.3,1.2,And 0.60 M,Respectively, Was introduced into a container at this temperature.Which of the following is true?

At 600?C, K_c = 2.8 for the reaction 2HgO(s) $f$ 2Hg(l)+ O₂(g) Calculate K at 600?C for this reaction.

The vapor pressure of acetic acid at 25?C is 16 Torr . ?G_r for the reaction CH₃COOH(l) $f$ CH₃COOH(g) At 25?C is

What is the relation between K and K_c for the reaction H₂(g)+ I₂(g)?2HI(g)

Given: 4NH₃(g)+ 5O₂(g) $f$ 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NH₃(g)+ $\frac { 5 } { 2 }$ O₂(g) $f$ 2NO(g)+ 3H₂O(g)