Question 1

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g)  2(g) + N2(g)    2NH3(g)  A) There will be no effect. B) More ammonia will be produced at the expense of hydrogen and nitrogen. C) Hydrogen and nitrogen will be produced at the expense of ammonia. D) The equilibrium constant will increase. E) The equilibrium constant will decrease." class="answers-bank-image d-inline" rel="preload" > 2NH3(g)

Accepted Answer

A)  There will be no effect.
B)  More ammonia will be produced at the expense of hydrogen and nitrogen.
C)  Hydrogen and nitrogen will be produced at the expense of ammonia.
D)  The equilibrium constant will increase.
E)  The equilibrium constant will decrease.F) All of the above
G) A) and B)

Question 2

Consider the reversible reaction: 2NO2(g)  2(g)    N2O4(g)  If the concentrations of both NO2 and N2O4 are each 0.016 M,what is the value of Qc? A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63" class="answers-bank-image d-inline" rel="preload" > N2O4(g)  If the concentrations of both NO2 and N2O4 are each 0.016 M,what is the value of Qc?

Accepted Answer

A)  0.016
B)  0.50
C)  1.0
D)  2.0
E)  63F) A) and C)
G) A) and E)

Question 3

Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g)  3(g)    Br2(g) + 3Cl2(g)  A) Kc = [Br2] [Cl2]/[BrCl3] B) Kc = [Br2] [Cl2]5/[BrCl3]2 C) Kc = [Br2] [Cl2]3/[BrCl3]2 D) Kc = [BrCl3]2/([Br2] × [Cl2]3)  E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3) " class="answers-bank-image d-inline" rel="preload" > Br2(g) + 3Cl2(g)

Accepted Answer

A)  Kc = [Br2] [Cl2]/[BrCl3]
B)  Kc = [Br2] [Cl2]5/[BrCl3]2
C)  Kc = [Br2] [Cl2]3/[BrCl3]2
D)  Kc = [BrCl3]2/([Br2] × [Cl2]3) 
E)  Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3) F) A) and E)
G) A) and D)

Question 4

Which substances are included in the equilibrium constant expression,Kc?

Accepted Answer

A)  Only pure solids
B)  Only pure liquids
C)  Only pure solids and liquids
D)  Only gases and dissolved substances
E)  All participating substancesF) A) and D)
G) C) and D)

Question 5

For the endothermic reaction A2(g)   2A(g) ,a snapshot of an equilibrium mixture of A(g) and A2(g) at low temperature may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.)   If the system pressure is lowered,what might the new equilibrium system look like?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) A) and B)
G) A) and C)

Question 6

A quantity of liquid methanol,CH3OH,is introduced into a rigid 3.00-L vessel,the vessel is sealed,and the temperature is raised to 500 K.At this temperature,the methanol vaporizes and decomposes according to the reaction CH3OH(g)  3OH,is introduced into a rigid 3.00-L vessel,the vessel is sealed,and the temperature is raised to 500 K.At this temperature,the methanol vaporizes and decomposes according to the reaction CH3OH(g)    CO(g) + 2H2(g) ,Kc = 6.90 ×10-2 If the concentration of H2 in the equilibrium mixture is 0.426 M,what mass of methanol was initially introduced into the vessel? A) 147 g B) 74.3 g C) 33.9 g D) 49.0 g E) 24.8 g" class="answers-bank-image d-inline" rel="preload" > CO(g) + 2H2(g) ,Kc = 6.90 ×10-2
If the concentration of H2 in the equilibrium mixture is 0.426 M,what mass of methanol was initially introduced into the vessel?

Accepted Answer

A)  147 g
B)  74.3 g
C)  33.9 g
D)  49.0 g
E)  24.8 gF) A) and B)
G) A) and C)

Question 7

At 250ºC,the equilibrium constant,KP,for the reaction PCl5(g)  P,for the reaction PCl5(g)    PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl5 after the system has reached equilibrium. A) 1.50 atm B) 1.24 atm C) 4.24 atm D) 0.94 atm E) 1.12 atm" class="answers-bank-image d-inline" rel="preload" > PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl5 after the system has reached equilibrium.

Accepted Answer

A)  1.50 atm
B)  1.24 atm
C)  4.24 atm
D)  0.94 atm
E)  1.12 atmF) A) and B)
G) None of the above

Question 8

The equilibrium constant KP at 427°C for the reaction N2(g) + 3H2(g)  P at 427°C for the reaction N2(g) + 3H2(g)    2NH3(g) is 9.4 ×10-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)  A) -33 kJ/mol B) -54 kJ/mol C) 54 kJ/mol D) 33 kJ/mol E) 1.3 J/mol" class="answers-bank-image d-inline" rel="preload" > 2NH3(g) is 9.4 ×10-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Accepted Answer

A)  -33 kJ/mol
B)  -54 kJ/mol
C)  54 kJ/mol
D)  33 kJ/mol
E)  1.3 J/molF) A) and E)
G) A) and D)

Question 9

Which statement is correct?

Accepted Answer

A)  When Q 
B)  When Q 
C)  When Q = K then ΔG = 0.
D)  When Q > K then ΔG = 1.
E)  When Q > K then ΔG = - RT.F) None of the above
G) A) and B)

Question 10

Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g)  2(g) + S2(g)    H2S(g) ; ΔH°rxn = -92 kJ/mol The equilibrium constant,KP,is 106 at 1023 K.Estimate the value of KP at 1218 K.(R = 8.314 J/K • mol)  A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598" class="answers-bank-image d-inline" rel="preload" > H2S(g) ; ΔH°rxn = -92 kJ/mol
The equilibrium constant,KP,is 106 at 1023 K.Estimate the value of KP at 1218 K.(R = 8.314 J/K • mol)

Accepted Answer

A)  5.05
B)  18.8
C)  34.7
D)  88.9
E)  598F) A) and E)
G) A) and B)

Question 11

Suppose 50.0 g of N2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N2O4(g)  2O4 is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N2O4(g)    2NO2(g) .For this reaction Kc = 0.133.Once the system has reached equilibrium,5.00 g of NO2 is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of NO2 in the final equilibrium mixture? A) 7.8 g B) 12.4 g C) 14.7 g D) 19.7 g E) 15.5 g" class="answers-bank-image d-inline" rel="preload" > 2NO2(g) .For this reaction Kc = 0.133.Once the system has reached equilibrium,5.00 g of NO2 is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of NO2 in the final equilibrium mixture?

Accepted Answer

A)  7.8 g
B)  12.4 g
C)  14.7 g
D)  19.7 g
E)  15.5 gF) A) and B)
G) A) and C)

Question 12

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr2 was 0.233 M.What is Kc for this reaction?
CO(g) + Br2(g)  2 was 0.233 M.What is Kc for this reaction? CO(g) + Br2(g)    COBr2(g)  A) 5.23 B) 2.14 C) 1.17 D) 0.467 E) 0.191" class="answers-bank-image d-inline" rel="preload" > COBr2(g)

Accepted Answer

A)  5.23
B)  2.14
C)  1.17
D)  0.467
E)  0.191F) All of the above
G) B) and E)

Question 13

Consider the equilibrium reaction: N2O4(g)  2O4(g)    2NO2(g)  Which of the following correctly describes the relationship between Kc and KP for the reaction? A) KP = Kc B) KP = RT × Kc C) KP = (RT × Kc ) -1 D) KP = Kc/RT E) KP = RT/Kc" class="answers-bank-image d-inline" rel="preload" > 2NO2(g)  Which of the following correctly describes the relationship between Kc and KP for the reaction?

Accepted Answer

A)  KP = Kc
B)  KP = RT × Kc
C)  KP = (RT × Kc ) -1
D)  KP = Kc/RT
E)  KP = RT/KcF) A) and B)
G) A) and C)

Question 14

The equilibrium constant,KP,has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g)  P,has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g)    2NOCl(g)  What is the value of Kc? (R = 0.08206 L • atm/K • mol)  A) 2.5 × 10-7 B) 6.5 × 10-4 C) 1.6 × 10-2 D) 1.7 E) None of these choices is correct." class="answers-bank-image d-inline" rel="preload" > 2NOCl(g) 
What is the value of Kc? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  2.5 × 10-7
B)  6.5 × 10-4
C)  1.6 × 10-2
D)  1.7
E)  None of these choices is correct.F) C) and E)
G) A) and B)

Question 15

Suppose 75.0 g of PCl5(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g)  5(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g)    PCl3(g) + Cl2(g)  If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)  A) 2.88 atm B) 2.28 atm C) 4.54 atm D) 7.43 atm E) 9.69 atm" class="answers-bank-image d-inline" rel="preload" > PCl3(g) + Cl2(g) 
If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

Accepted Answer

A)  2.88 atm
B)  2.28 atm
C)  4.54 atm
D)  7.43 atm
E)  9.69 atmF) D) and E)
G) A) and B)

Question 16

If,in a particular process,reactants are able to form products,and products are also able to form reactants,then this process may be described as

Accepted Answer

A)  a reversible process.
B)  an elementary process.
C)  at equilibrium.
D)  forbidden.
E)  a forward process.F) C) and D)
G) B) and D)

Question 17

If the system 3H2(g)+ N2(g)
 2NH3(g)is at equilibrium and more N2 is added,a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.

Accepted Answer

A) True 
 B)False

Question 18

In the gas phase,formic acid forms a dimer,2HCOOH(g)  2(g) .For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (KP) for this reaction at 75 °C. A) 8960 B) 273 C) 0.120 D) 8.33 E) 1.12 × 10-4" class="answers-bank-image d-inline" rel="preload" > (HCOOH) 2(g) .For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (KP) for this reaction at 75 °C.

Accepted Answer

A)  8960
B)  273
C)  0.120
D)  8.33
E)  1.12 × 10-4F) B) and D)
G) B) and E)

Question 19

When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________________.

Accepted Answer

The answer of When the concentrations of both the reactants...

Question 20

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br2 :1.59 atm; NOBr: 7.68 atm.Calculate KP for the reaction. 2NO(g) + Br2(g)  2 :1.59 atm; NOBr: 7.68 atm.Calculate KP for the reaction. 2NO(g) + Br2(g)    2NOBr(g)  A) 7.45 × 10-3 B) 0.109 C) 9.18 D) 91.8 E) 134" class="answers-bank-image d-inline" rel="preload" > 2NOBr(g)

Accepted Answer

A)  7.45 × 10-3
B)  0.109
C)  9.18
D)  91.8
E)  134F) B) and E)
G) C) and D)

Exam 15: Chemical Equilibrium

When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________________.

Correct Answer
verified

Correct Answer
verified

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr₂ was 0.233 M.What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Correct Answer
verified

Suppose 75.0 g of PCl₅(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g) + Cl₂(g) If K_P = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

Correct Answer
verified

Correct Answer
verified

The equilibrium constant,K_P,has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ :1.59 atm; NOBr: 7.68 atm.Calculate K_P for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g) + 3Cl₂(g)

Correct Answer
verified

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

Correct Answer
verified

Which statement is correct?

Correct Answer
verified

At 250ºC,the equilibrium constant,K_P,for the reaction PCl⁵(g) PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
verified

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added,a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

Correct Answer
verified

If,in a particular process,reactants are able to form products,and products are also able to form reactants,then this process may be described as

Correct Answer
verified

The equilibrium constant K_P at 427°C for the reaction N₂(g) + 3H₂(g) 2NH₃(g) is 9.4 ×10^-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Correct Answer
verified

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

Correct Answer
verified

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH) ₂(g) .For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (K_P) for this reaction at 75 °C.

Correct Answer
verified

For the endothermic reaction A2(g) 2A(g) ,a snapshot of an equilibrium mixture of A(g) and A2(g) at low temperature may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) If the system pressure is lowered,what might the new equilibrium system look like?

Correct Answer
verified

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M,what is the value of Q_c?

Correct Answer
verified

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) ; ΔH°_rxn = -92 kJ/mol The equilibrium constant,K_P,is 106 at 1023 K.Estimate the value of K_P at 1218 K.(R = 8.314 J/K • mol)

Correct Answer
verified

Which substances are included in the equilibrium constant expression,K_c?

Correct Answer
verified

Exam 15: Chemical Equilibrium

When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________________.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr2 was 0.233 M.What is Kc for this reaction? CO(g) + Br2(g) COBr2(g)

Correct AnswerverifiedShow Answer

Suppose 75.0 g of PCl5(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g) + Cl2(g) If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The equilibrium constant,KP,has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) 2NOCl(g) What is the value of Kc? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br2 :1.59 atm; NOBr: 7.68 atm.Calculate KP for the reaction. 2NO(g) + Br2(g) 2NOBr(g)

Correct AnswerverifiedShow Answer

Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Br2(g) + 3Cl2(g)

Correct AnswerverifiedShow Answer

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2NH3(g)

Correct AnswerverifiedShow Answer

Which statement is correct?

Correct AnswerverifiedShow Answer

At 250ºC,the equilibrium constant,KP,for the reaction PCl5(g) PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl5 after the system has reached equilibrium.

Correct AnswerverifiedShow Answer

If the system 3H2(g)+ N2(g) 2NH3(g)is at equilibrium and more N2 is added,a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.

Correct AnswerverifiedShow Answer

If,in a particular process,reactants are able to form products,and products are also able to form reactants,then this process may be described as

Correct AnswerverifiedShow Answer

The equilibrium constant KP at 427°C for the reaction N2(g) + 3H2(g) 2NH3(g) is 9.4 ×10-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and KP for the reaction?

Correct AnswerverifiedShow Answer

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH) 2(g) .For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (KP) for this reaction at 75 °C.

Correct AnswerverifiedShow Answer

For the endothermic reaction A2(g) 2A(g) ,a snapshot of an equilibrium mixture of A(g) and A2(g) at low temperature may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) If the system pressure is lowered,what might the new equilibrium system look like?

Correct AnswerverifiedShow Answer

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are each 0.016 M,what is the value of Qc?

Correct AnswerverifiedShow Answer

Hydrogen sulfide can be formed in the following reaction: H2(g) + S2(g) H2S(g) ; ΔH°rxn = -92 kJ/mol The equilibrium constant,KP,is 106 at 1023 K.Estimate the value of KP at 1218 K.(R = 8.314 J/K • mol)

Correct AnswerverifiedShow Answer

Which substances are included in the equilibrium constant expression,Kc?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr₂ was 0.233 M.What is K_c for this reaction? CO(g) + Br₂(g) COBr₂(g)

Correct Answer
verified

Suppose 75.0 g of PCl₅(g) is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g) + Cl₂(g) If K_P = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

Correct Answer
verified

Correct Answer
verified

The equilibrium constant,K_P,has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ :1.59 atm; NOBr: 7.68 atm.Calculate K_P for the reaction. 2NO(g) + Br₂(g) 2NOBr(g)

Correct Answer
verified

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g) + 3Cl₂(g)

Correct Answer
verified

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H₂(g) + N₂(g) 2NH₃(g)

Correct Answer
verified

Correct Answer
verified

At 250ºC,the equilibrium constant,K_P,for the reaction PCl⁵(g) PCl₃(g) + Cl₂(g) is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
verified

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added,a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

Correct Answer
verified

Correct Answer
verified

The equilibrium constant K_P at 427°C for the reaction N₂(g) + 3H₂(g) 2NH₃(g) is 9.4 ×10^-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Correct Answer
verified

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

Correct Answer
verified

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH) ₂(g) .For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (K_P) for this reaction at 75 °C.

Correct Answer
verified

Correct Answer
verified

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M,what is the value of Q_c?

Correct Answer
verified

Hydrogen sulfide can be formed in the following reaction: H₂(g) + S₂(g) H₂S(g) ; ΔH°_rxn = -92 kJ/mol The equilibrium constant,K_P,is 106 at 1023 K.Estimate the value of K_P at 1218 K.(R = 8.314 J/K • mol)

Correct Answer
verified

Which substances are included in the equilibrium constant expression,K_c?

Correct Answer
verified