Question 1

The effect of a volume decrease on the reaction
C(s)+ H2O(g) 
$f$
CO(g)+ H2(g)
Is

Accepted Answer

A)  that K decreases. 
B)  more CO(g) and H2(g) are produced. 
C)  no change. 
D)  more H2O(g) is produced. 
E)  that K increases. 
A)  that K decreases. 
B)  more CO(g) and H2(g) are produced. 
C)  no change. 
D)  more H2O(g) is produced. 
E)  that K increases.

Question 2

the van't Hoff i of HF differs from that of HCl?

Accepted Answer

A) True 
 B)False

Question 3

Calculate the equilibrium constant for the following reaction at 25F1F1F1S1?F1F1F10C
2TiCl3(s)+ 2HCl(g)F1S1S1W1?F1F1F10 2TiCl4(g)+ H2(g)
Given F1F1F1S1?F1F1F10GF1F1F1S1?F1F1F10 = +46.6 kJ.

Accepted Answer

A)  3.8 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1098  
B)  1.5 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1019  
C)  6.7 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F109  
D)  6.6 F1F1F1S1*F1F1F10 1018  
E)  1.5 F1F1F1S1*F1F1F10 108  
A)  3.8 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1098  
B)  1.5 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F1019  
C)  6.7 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F109  
D)  6.6 F1F1F1S1*F1F1F10 1018  
E)  1.5 F1F1F1S1*F1F1F10 108

Question 4

Of the following, which would likely dissolve in toluene?

Accepted Answer

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

Question 5

Because a solute increases the entropy of the liquid phase while the enthalpy is left unchanged,there is a decrease in the molar free energy of the solvent.

Accepted Answer

A) True 
 B)False

Question 6

Calculate the molality of ethanol in a solution of water,given that the mole fraction of ethanol is 0.300.

Accepted Answer

The answer of Calculate the molality of ethanol in a...

Question 7

Consider the reaction
3Fe(s)+ 4H2O(g) $f$
4H2(g)+ Fe3O4(s)
If the volume of the container is reduced,

Accepted Answer

A)  the equilibrium constant increases. 
B)  more H2(g) is produced. 
C)  no change occurs. 
D)  more H2O(g) is produced. 
E)  more Fe(s) is produced. 
A)  the equilibrium constant increases. 
B)  more H2(g) is produced. 
C)  no change occurs. 
D)  more H2O(g) is produced. 
E)  more Fe(s) is produced.

Question 8

When three phases are in mutual equilibrium,such as at the triple point of water,the degrees of freedom equal 0.

Accepted Answer

A) True 
 B)False

Question 9

Rank the following species in order of increasing vapor pressure at 25$\omicron$C.
water,diethyl ether,ethanol,mercury

Accepted Answer

mercury <

Question 10

The phase diagram for sulfur is given below.    Which of the following is true?

Accepted Answer

A)  Sulfur has 2 triple points. 
B)  Monoclinic sulfur does not sublime. 
C)  Sulfur has 0 triple points. 
D)  Sulfur has 3 triple points. 
E)  Rhombic sulfur cannot be directly converted to liquid. 
A)  Sulfur has 2 triple points. 
B)  Monoclinic sulfur does not sublime. 
C)  Sulfur has 0 triple points. 
D)  Sulfur has 3 triple points. 
E)  Rhombic sulfur cannot be directly converted to liquid.

Question 11

A plot of ln(vapor pressure) versus 1/T for methanol gives a straight line with an intercept of 13.6.The enthalpy of vaporization of methanol is

Accepted Answer

A)  113 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
B)  13.6 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
C)  611 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
D)  1.64 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
E)  Not enough information given to calculate. 
A)  113 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
B)  13.6 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
C)  611 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
D)  1.64 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101. 
E)  Not enough information given to calculate.

Question 12

The normal boiling point of ethanol is 78$\omicron$C.If the vapor pressure of ethanol is 13.3 kPa at 34.9$\omicron$C,calculate the enthalpy of vaporization of ethanol.

Accepted Answer

Question 13

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 F1F1F1S1*F1F1F1010F1F1F1S1-F1F1F106 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,F1F1F1S1?F1F1F10HF1F1F1S1?F1F1F10 = 92.38 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101.

Accepted Answer

A)  241 K 
B)  332 K 
C)  59 K 
D)  390 K 
E)  117 K 
A)  241 K 
B)  332 K 
C)  59 K 
D)  390 K 
E)  117 K

Question 14

The phase diagram for a pure substance is given below .
The solid sublimes

Accepted Answer

A)  at 400 K and 200 atm. 
B)  at 200 K and 100 atm. 
C)  at 300 K and 100 atm. 
D)  at 300 K and 75 atm. 
E)  if warmed at any pressure below 50 atm. 
A)  at 400 K and 200 atm. 
B)  at 200 K and 100 atm. 
C)  at 300 K and 100 atm. 
D)  at 300 K and 75 atm. 
E)  if warmed at any pressure below 50 atm.

Question 15

Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the significance of the slopes of the solid-liquid lines.

Accepted Answer

For water,the solid is less de

Question 16

If a 1-L flask containing D2(g),N2(g),and ND3(g)at equilibrium at 300 K and a 1-L flask of H2(g),N2(g),and NH3(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD2(g),and NH2D(g)are also present.What conclusion(s)can be drawn?

Accepted Answer

Equilibriu

Question 17

Consider the following reaction at a certain temperature:
PCl5(g)
$f$
PCl3(g)+ Cl2(g)
Kc = 0.100
At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl5(g),PCl3(g),And Cl2(g)Is added,What is the equilibrium concentration of Cl2(g)?

Accepted Answer

A)  3.0 M 
B)  essentially zero 
C)  0.65 M 
D)  2.75 M 
E)  3.35 M 
A)  3.0 M 
B)  essentially zero 
C)  0.65 M 
D)  2.75 M 
E)  3.35 M

Question 18

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 F1F1F1S1*F1F1F10 10F1F1F1S1-F1F1F106 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,F1F1F1S1?F1F1F10HF1F1F1S1?F1F1F10 = 92.38 kJF1F1F1S1.F1F1F10molF1F1F1S1-F1F1F101.

Accepted Answer

A)  193 K 
B)  353 K 
C)  466 K 
D)  492 K 
E)  219 K 
A)  193 K 
B)  353 K 
C)  466 K 
D)  492 K 
E)  219 K

Question 19

The critical temperature of N2 is F1F1F1S1-F1F1F10147oC.Nitrogen gas cannot be converted to liquid nitrogen at F1F1F1S1-F1F1F1073oC,even at extremely high pressures.

Accepted Answer

A) True 
 B)False

Question 20

In a pressure cooker,the boiling point of water is less than 100$\omicron$C.

Accepted Answer

A) True 
 B)False

The effect of a volume decrease on the reaction C(s)+ H₂O(g) $f$ CO(g)+ H₂(g) Is

the van't Hoff i of HF differs from that of HCl?

Calculate the equilibrium constant for the following reaction at 25?C 2TiCl₃(s)+ 2HCl(g)? 2TiCl₄(g)+ H₂(g) Given ?G? = +46.6 kJ.

Of the following, which would likely dissolve in toluene?

Because a solute increases the entropy of the liquid phase while the enthalpy is left unchanged,there is a decrease in the molar free energy of the solvent.

Calculate the molality of ethanol in a solution of water,given that the mole fraction of ethanol is 0.300.

Consider the reaction 3Fe(s)+ 4H₂O(g) $f$ 4H₂(g)+ Fe₃O₄(s) If the volume of the container is reduced,

When three phases are in mutual equilibrium,such as at the triple point of water,the degrees of freedom equal 0.

Rank the following species in order of increasing vapor pressure at 25^$\omicron$C. water,diethyl ether,ethanol,mercury

The phase diagram for sulfur is given below. Which of the following is true?

A plot of ln(vapor pressure) versus 1/T for methanol gives a straight line with an intercept of 13.6.The enthalpy of vaporization of methanol is

The normal boiling point of ethanol is 78^$\omicron$C.If the vapor pressure of ethanol is 13.3 kPa at 34.9^$\omicron$C,calculate the enthalpy of vaporization of ethanol.

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 *10^-⁶ at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,?H? = 92.38 kJ.mol^-¹.

The phase diagram for a pure substance is given below . The solid sublimes

Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the significance of the slopes of the solid-liquid lines.

If a 1-L flask containing D₂(g),N₂(g),and ND₃(g)at equilibrium at 300 K and a 1-L flask of H₂(g),N₂(g),and NH₃(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD₂(g),and NH₂D(g)are also present.What conclusion(s)can be drawn?

Consider the following reaction at a certain temperature: PCl₅(g) $f$ PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₅(g),PCl₃(g),And Cl₂(g)Is added,What is the equilibrium concentration of Cl₂(g)?

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 * 10^-⁶ at 298 K.Calculate the temperature at which K = 1.00.For this reaction,?H? = 92.38 kJ.mol^-¹.

The critical temperature of N₂ is -147^oC.Nitrogen gas cannot be converted to liquid nitrogen at -73^oC,even at extremely high pressures.

In a pressure cooker,the boiling point of water is less than 100^$\omicron$C.

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Exam 5: Equilibrium

The effect of a volume decrease on the reaction C(s)+ H2O(g) fff CO(g)+ H2(g) Is

the van't Hoff i of HF differs from that of HCl?

Calculate the equilibrium constant for the following reaction at 25?C 2TiCl3(s)+ 2HCl(g)? 2TiCl4(g)+ H2(g) Given ?G? = +46.6 kJ.

Of the following, which would likely dissolve in toluene?

Because a solute increases the entropy of the liquid phase while the enthalpy is left unchanged,there is a decrease in the molar free energy of the solvent.

Calculate the molality of ethanol in a solution of water,given that the mole fraction of ethanol is 0.300.

Consider the reaction 3Fe(s)+ 4H2O(g) fff 4H2(g)+ Fe3O4(s) If the volume of the container is reduced,

When three phases are in mutual equilibrium,such as at the triple point of water,the degrees of freedom equal 0.

Rank the following species in order of increasing vapor pressure at 25 ο\omicronο C. water,diethyl ether,ethanol,mercury

The phase diagram for sulfur is given below. Which of the following is true?

A plot of ln(vapor pressure) versus 1/T for methanol gives a straight line with an intercept of 13.6.The enthalpy of vaporization of methanol is

The normal boiling point of ethanol is 78 ο\omicronο C.If the vapor pressure of ethanol is 13.3 kPa at 34.9 ο\omicronο C,calculate the enthalpy of vaporization of ethanol.

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 *10-6 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,?H? = 92.38 kJ.mol-1.

The phase diagram for a pure substance is given below . The solid sublimes

Consider the phase diagrams for water and carbon dioxide given in the text on page 315.Explain the significance of the slopes of the solid-liquid lines.

If a 1-L flask containing D2(g),N2(g),and ND3(g)at equilibrium at 300 K and a 1-L flask of H2(g),N2(g),and NH3(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD2(g),and NH2D(g)are also present.What conclusion(s)can be drawn?

Consider the following reaction at a certain temperature: PCl5(g) fff PCl3(g)+ Cl2(g) Kc = 0.100 At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl5(g),PCl3(g),And Cl2(g)Is added,What is the equilibrium concentration of Cl2(g)?

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 * 10-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,?H? = 92.38 kJ.mol-1.

The critical temperature of N2 is -147oC.Nitrogen gas cannot be converted to liquid nitrogen at -73oC,even at extremely high pressures.

In a pressure cooker,the boiling point of water is less than 100 ο\omicronο C.

Atoms

Molecules

States of Matter

Thermodynamics

Reactions

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

The effect of a volume decrease on the reaction C(s)+ H₂O(g) $f$ CO(g)+ H₂(g) Is

Calculate the equilibrium constant for the following reaction at 25?C 2TiCl₃(s)+ 2HCl(g)? 2TiCl₄(g)+ H₂(g) Given ?G? = +46.6 kJ.

Consider the reaction 3Fe(s)+ 4H₂O(g) $f$ 4H₂(g)+ Fe₃O₄(s) If the volume of the container is reduced,

Rank the following species in order of increasing vapor pressure at 25^$\omicron$C. water,diethyl ether,ethanol,mercury

The normal boiling point of ethanol is 78^$\omicron$C.If the vapor pressure of ethanol is 13.3 kPa at 34.9^$\omicron$C,calculate the enthalpy of vaporization of ethanol.

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 *10^-⁶ at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,?H? = 92.38 kJ.mol^-¹.

If a 1-L flask containing D₂(g),N₂(g),and ND₃(g)at equilibrium at 300 K and a 1-L flask of H₂(g),N₂(g),and NH₃(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD₂(g),and NH₂D(g)are also present.What conclusion(s)can be drawn?

Consider the following reaction at a certain temperature: PCl₅(g) $f$ PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₅(g),PCl₃(g),And Cl₂(g)Is added,What is the equilibrium concentration of Cl₂(g)?

For the decomposition of ammonia to nitrogen and hydrogen, the equilibrium constant is 1.47 * 10^-⁶ at 298 K.Calculate the temperature at which K = 1.00.For this reaction,?H? = 92.38 kJ.mol^-¹.

The critical temperature of N₂ is -147^oC.Nitrogen gas cannot be converted to liquid nitrogen at -73^oC,even at extremely high pressures.

In a pressure cooker,the boiling point of water is less than 100^$\omicron$C.