Question 1

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g) + 1/2O2(g)  4(g) + 1/2O2(g)       COCl2(g) + Cl2(g) , Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g)       2COCl2(g) + 2Cl2(g) . A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10" class="answers-bank-image d-inline" rel="preload" >  
 COCl2(g) + Cl2(g) , Kc = 4.4 * 109 at 1,000 K
Calculate Kc for the reaction 2CCl4(g) + O2(g)  4(g) + 1/2O2(g)       COCl2(g) + Cl2(g) , Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g)       2COCl2(g) + 2Cl2(g) . A) 4.4 * 109 B) 8.8 * 109 C) 1.9 * 1010 D) 1.9 * 1019 E) 2.3 * 10-10" class="answers-bank-image d-inline" rel="preload" >  
 2COCl2(g) + 2Cl2(g) .

Accepted Answer

A)  4.4 * 109
B)  8.8 * 109
C)  1.9 * 1010
D)  1.9 * 1019
E)  2.3 * 10-10F) A) and E)
G) B) and E)

Question 2

Consider the two gaseous equilibria: 
1 and K2 are related by A) K2 = K12 B) K22 = K1 C) K2 = 1/K   D) K2 = 1/K1 E) none of these." class="answers-bank-image d-inline" rel="preload" >
The values of the equilibrium constants K1 and K2 are related by

Accepted Answer

A)  K2 = K12
B)  K22 = K1
C)  K2 = 1/K 1 and K2 are related by 
A)  K2 = K12 
B)  K22 = K1 
C)  K2 = 1/K   
D)  K2 = 1/K1 
E)  none of these." class="answers-bank-image d-inline" rel="preload" >
D)  K2 = 1/K1
E)  none of these.F) A) and E)
G) D) and E)

Question 3

Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g)  2, a poisonous gas, decomposes according to the equation COCl2(g)       CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC. A) 0.125 B) 8.0 C) 6.1 D) 0.16 E) 0.083" class="answers-bank-image d-inline" rel="preload" >    CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

Accepted Answer

A)  0.125
B)  8.0
C)  6.1
D)  0.16
E)  0.083F) D) and E)
G) B) and D)

Question 4

Calculate Kc for the reaction 2HI(g)     c for the reaction 2HI(g)          H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L. A) 5.25 B) 0.22 C) 4.5 D) 0.19 E) 1.6 * 102" class="answers-bank-image d-inline" rel="preload" >  
 H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Accepted Answer

A)  5.25
B)  0.22
C)  4.5
D)  0.19
E)  1.6 * 102F) C) and D)
G) B) and C)

Question 5

Hydrogen iodide decomposes according to the equation:
2HI(g)   
H2(g)+ I2(g), Kc = 0.0156 at 400ºC
A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC.
Calculate the concentration of HI at equilibrium.

Accepted Answer

Question 6

The equilibrium constant for the chemical equation
2NO(g)+ O2(g)   
2NO2(g)
is two times the equilibrium constant for the chemical equation
NO(g)+ 1/2O2(g)   
NO2(g).

Accepted Answer

A) True 
 B)False

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.Calculate the 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.Calculate the 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 E)
G) A) and B)

Question 8

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J   
CO(g)+ H2(g).If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

Accepted Answer

The temper...

Question 9

Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Accepted Answer

A catalyst affects both the fo...

Question 10

For the reaction SO2(g) + NO2(g)  2(g) + NO2(g)      SO3(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20.L container, what concentration of SO3 will be present at equilibrium? A) 0.48 mol/L B) 0.11 mol/L C) 0.95 mol/L D) 2.22 mol/L E) 18 mol/L" class="answers-bank-image d-inline" rel="preload" >   SO3(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20.L container, what concentration of SO3 will be present at equilibrium?

Accepted Answer

A)  0.48 mol/L
B)  0.11 mol/L
C)  0.95 mol/L
D)  2.22 mol/L
E)  18 mol/LF) A) and D)
G) C) and D)

Question 11

Which of these statements is true about chemical equilibria in general?

Accepted Answer

A)  At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants].
B)  Equilibrium is the result of the cessation of all chemical change.
C)  There is only one set of equilibrium concentrations that equals the Kc value.
D)  At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction.
E)  At equilibrium, the rate of the forward reaction is equal to as the rate of the reverse reaction.F) A) and D)
G) B) and C)

Question 12

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2(aq) + H2O(l)  2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? A)    B) Kc =   C) Kc =   D) Kc =   E) Kc =  " class="answers-bank-image d-inline" rel="preload" >  
 H2CO3(aq) 
Which one of the following is the correct equilibrium constant expression (Kc) for this reaction?

Accepted Answer

A)   2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? 
A)     
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
B)  Kc = 2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? 
A)     
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
C)  Kc = 2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? 
A)     
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
D)  Kc = 2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? 
A)     
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >
E)  Kc = 2(aq) + H2O(l)       H2CO3(aq)  Which one of the following is the correct equilibrium constant expression (Kc) for this reaction? 
A)     
B)  Kc =   
C)  Kc =   
D)  Kc =   
E)  Kc =  " class="answers-bank-image d-inline" rel="preload" >F) B) and E)
G) None of the above

Question 13

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H2(g)  2(g)      H2O(g) + Cu(s)  \Delta Hºrxn = -2.0 kJ/mol A) increasing the pressure by means of a moving piston at constant T. B) increasing the pressure by adding an inert gas such as nitrogen. C) decreasing the temperature. D) allowing some gases to escape at constant P and T. E) adding a catalyst. " class="answers-bank-image d-inline" rel="preload" >  
H2O(g) + Cu(s)  Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

Accepted Answer

A)  increasing the pressure by means of a moving piston at constant T.
B)  increasing the pressure by adding an inert gas such as nitrogen.
C)  decreasing the temperature.
D)  allowing some gases to escape at constant P and T.
E)  adding a catalyst. F) A) and B)
G) C) and D)

Question 14

Consider the following equilibrium,
4NH3(g)+ 3O2(g)   
2N2(g)+ 6H2O(g)+ 1531 kJ
State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Accepted Answer

Question 15

On analysis, an equilibrium mixture for the reaction 2H2S(g)  2S(g)       2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. A) 1.6 B) 3.2 C) 12.8 D) 0.64 E) 0.8" class="answers-bank-image d-inline" rel="preload" >    2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

Accepted Answer

A)  1.6
B)  3.2
C)  12.8
D)  0.64
E)  0.8F) A) and D)
G) A) and E)

Question 16

If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g)  2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g)       2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2. A) 0.152 atm B) 0.174 atm C) 0.200 atm D) 0.326 atm E) The total pressure cannot be calculated because Kp is not given" class="answers-bank-image d-inline" rel="preload" >    2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2.

Accepted Answer

A)  0.152 atm
B)  0.174 atm
C)  0.200 atm
D)  0.326 atm
E)  The total pressure cannot be calculated because Kp is not givenF) B) and E)
G) A) and B)

Question 17

The reaction A(g) + 2B(g)     C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction. A) 0.060 B) 5.1 C) 17 D) 19 E) 25" class="answers-bank-image d-inline" rel="preload" >    C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction.

Accepted Answer

A)  0.060
B)  5.1
C)  17
D)  19
E)  25F) A) and C)
G) None of the above

Question 18

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g)  2 concentration to increase? 2NOBr(g)      2NO(g) + Br2(g) ,  \Delta Hºrxn= 30 kJ/mol A) Lower the temperature. B) Remove some NO. C) Remove some NOBr. D) Compress the gas mixture into a smaller volume. " class="answers-bank-image d-inline" rel="preload" >  
2NO(g) + Br2(g) ,  Δ\DeltaΔ Hºrxn= 30 kJ/mol

Accepted Answer

A)  Lower the temperature.
B)  Remove some NO.
C)  Remove some NOBr.
D)  Compress the gas mixture into a smaller volume. E) None of the above
F) A) and D)

Question 19

Consider the following reactions and their associated equilibrium constants: 
c, A) Kc = K1 + K2 B) Kc = K1/K2 C) Kc = K1  - K2 D) Kc = (K1) (K2)  E) Kc = K2/K1" class="answers-bank-image d-inline" rel="preload" >
For the reaction A + 2B c, A) Kc = K1 + K2 B) Kc = K1/K2 C) Kc = K1  - K2 D) Kc = (K1) (K2)  E) Kc = K2/K1" class="answers-bank-image d-inline" rel="preload" >D + E, having equilibrium constant Kc,

Accepted Answer

A)  Kc = K1 + K2
B)  Kc = K1/K2
C)  Kc = K1  - K2
D)  Kc = (K1) (K2) 
E)  Kc = K2/K1F) All of the above
G) C) and D)

Question 20

Kc for the reaction CO2(g)+ H2(g)   
H2O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Accepted Answer

Exam 14: Chemical Equilibrium

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

Consider the following reactions and their associated equilibrium constants: For the reaction A + 2B D + E, having equilibrium constant K_c,

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
verified

On analysis, an equilibrium mixture for the reaction 2H₂S(g) 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

Correct Answer
verified

K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct Answer
verified

For the reaction SO₂(g) + NO₂(g) SO₃(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20.L container, what concentration of SO₃ will be present at equilibrium?

Correct Answer
verified

Consider the two gaseous equilibria: The values of the equilibrium constants K₁ and K₂are related by

Correct Answer
verified

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate K_c for this reaction.

Correct Answer
verified

Which of these statements is true about chemical equilibria in general?

Correct Answer
verified

The equilibrium constant for the chemical equation 2NO(g)+ O₂(g) 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g)+ ¹/₂O₂(g) NO₂(g).

Correct Answer
verified

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq) + H₂O(l) H₂CO₃(aq) Which one of the following is the correct equilibrium constant expression (K_c) for this reaction?

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.Calculate the pressure of PCl₅ after the system has reached equilibrium.

Correct Answer
verified

Correct Answer
verified

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

Correct Answer
verified
The temper...
View Answer

If one starts with pure NO₂(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO₂(g) 2NO(g) + O₂(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO₂.

Correct Answer
verified

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g) + ¹/₂O₂(g) COCl₂(g) + Cl₂(g) , K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g) + O₂(g) 2COCl₂(g) + 2Cl₂(g) .

Correct Answer
verified

Hydrogen iodide decomposes according to the equation: 2HI(g) H₂(g)+ I₂(g), K_c = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of HI at equilibrium.

Correct Answer
verified

Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Correct Answer
verified
A catalyst affects both the fo...
View Answer

Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

Correct Answer
verified

Exam 14: Chemical Equilibrium

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br2 concentration to increase? 2NOBr(g) 2NO(g) + Br2(g) , Δ\DeltaΔ Hºrxn= 30 kJ/mol

Correct AnswerverifiedShow Answer

Calculate Kc for the reaction 2HI(g) H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27 mol/L.

Correct AnswerverifiedShow Answer

Consider the following reactions and their associated equilibrium constants: For the reaction A + 2B D + E, having equilibrium constant Kc,

Correct AnswerverifiedShow Answer

Consider the following equilibrium, 4NH3(g)+ 3O2(g) 2N2(g)+ 6H2O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct AnswerverifiedShow Answer

On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction.

Correct AnswerverifiedShow Answer

Kc for the reaction CO2(g)+ H2(g) H2O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct AnswerverifiedShow Answer

For the reaction SO2(g) + NO2(g) SO3(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO2 and 2.0 moles of NO2 are placed in a 20.L container, what concentration of SO3 will be present at equilibrium?

Correct AnswerverifiedShow Answer

Consider the two gaseous equilibria: The values of the equilibrium constants K1 and K2 are related by

Correct AnswerverifiedShow Answer

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction.

Correct AnswerverifiedShow Answer

Which of these statements is true about chemical equilibria in general?

Correct AnswerverifiedShow Answer

The equilibrium constant for the chemical equation 2NO(g)+ O2(g) 2NO2(g) is two times the equilibrium constant for the chemical equation NO(g)+ 1/2O2(g) NO2(g).

Correct AnswerverifiedShow Answer

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2(aq) + H2O(l) H2CO3(aq) Which one of the following is the correct equilibrium constant expression (Kc) for this reaction?

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.Calculate the pressure of PCl5 after the system has reached equilibrium.

Correct AnswerverifiedShow Answer

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H2(g) H2O(g) + Cu(s) Δ\DeltaΔ Hºrxn = -2.0 kJ/mol

Correct AnswerverifiedShow Answer

Consider the equilibrium equation C(s)+ H2O(g)+ 2296 J CO(g)+ H2(g).If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

Correct AnswerverifiedThe temper...View AnswerShow Answer

If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g) 2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2.

Correct AnswerverifiedShow Answer

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g) + 1/2O2(g) COCl2(g) + Cl2(g) , Kc = 4.4 * 109 at 1,000 K Calculate Kc for the reaction 2CCl4(g) + O2(g) 2COCl2(g) + 2Cl2(g) .

Correct AnswerverifiedShow Answer

Hydrogen iodide decomposes according to the equation: 2HI(g) H2(g)+ I2(g), Kc = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of HI at equilibrium.

Correct AnswerverifiedShow Answer

Describe why addition of a catalyst does not affect the equilibrium constant for a reaction.

Correct AnswerverifiedA catalyst affects both the fo...View AnswerShow Answer

Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g) CO(g) + Cl2(g) . Calculate Kp for this reaction if Kc = 0.083 at 900ºC.

Correct AnswerverifiedShow Answer

Correct Answer
verified

Calculate K_c for the reaction 2HI(g) H₂(g) + I₂(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I₂] = 0.60 mol/L, [H₂] = 0.27 mol/L.

Correct Answer
verified

Consider the following reactions and their associated equilibrium constants: For the reaction A + 2B D + E, having equilibrium constant K_c,

Correct Answer
verified

Consider the following equilibrium, 4NH₃(g)+ 3O₂(g) 2N₂(g)+ 6H₂O(g)+ 1531 kJ State whether the concentrations of the products would increase, decrease, or remain constant when the temperature is increased.

Correct Answer
verified

On analysis, an equilibrium mixture for the reaction 2H₂S(g) 2H₂(g) + S₂(g) was found to contain 1.0 mol H₂S, 4.0 mol H₂, and 0.80 mol S₂ in a 4.0 L vessel. Calculate the equilibrium constant, K_c, for this reaction.

Correct Answer
verified

K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC.Calculate the number of moles of carbon monoxide in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Correct Answer
verified

For the reaction SO₂(g) + NO₂(g) SO₃(g) + NO(g) , the equilibrium constant is 18.0 at 1,200ºC. If 1.0 mole of SO₂ and 2.0 moles of NO₂ are placed in a 20.L container, what concentration of SO₃ will be present at equilibrium?

Correct Answer
verified

Consider the two gaseous equilibria: The values of the equilibrium constants K₁ and K₂are related by

Correct Answer
verified

The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate K_c for this reaction.

Correct Answer
verified

Correct Answer
verified

The equilibrium constant for the chemical equation 2NO(g)+ O₂(g) 2NO₂(g) is two times the equilibrium constant for the chemical equation NO(g)+ ¹/₂O₂(g) NO₂(g).

Correct Answer
verified

The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO₂(aq) + H₂O(l) H₂CO₃(aq) Which one of the following is the correct equilibrium constant expression (K_c) for this reaction?

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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.Calculate the pressure of PCl₅ after the system has reached equilibrium.

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Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g).If additional gaseous water is added to this reaction mixture, what will happen to the temperature of the mixture?

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The temper...
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If one starts with pure NO₂(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO₂(g) 2NO(g) + O₂(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO₂.

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Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g) + ¹/₂O₂(g) COCl₂(g) + Cl₂(g) , K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g) + O₂(g) 2COCl₂(g) + 2Cl₂(g) .

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Hydrogen iodide decomposes according to the equation: 2HI(g) H₂(g)+ I₂(g), K_c = 0.0156 at 400ºC A 0.660 mol sample of HI was injected into a 2.00 L reaction vessel held at 400ºC. Calculate the concentration of HI at equilibrium.

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A catalyst affects both the fo...
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Phosgene, COCl₂, a poisonous gas, decomposes according to the equation COCl₂(g) CO(g) + Cl₂(g) . Calculate K_p for this reaction if K_c = 0.083 at 900ºC.

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