Question 1 (2 points) Write the equilibrium expression for H2O(g) + CO(g) H2(g)

Question

Question 1 (2 points)
Write the equilibrium expression for H2O(g) + CO(g) H2(g) + CO2(g)
Question 1 options:
1- Kc = [CO2] [H2] / [H2O] [CO]
2- Kc = [H2O] [CO] / [CO2] [H2]
3- Kc = [CO2] [H2] / [CO]
4- none

Question 2 (2 point)
What is n for the following equation in relating Kc to Kp?
N2(g) + 3 H2(g) 2 NH3(g)
Question 2 options:

2
4
-2
-4

Question 3 (3 points)
The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500 K?
N2(g) + 3 H2(g) 2 NH3(g)

Question 3 options:
61
3.6 × 10-2
1.9 × 10-2
15
28

Question 4 (3 points)
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.
2 N2(g) + O2(g) 2 N2O(g)

Question 4 options:
2.2 × 10-19
4.5 × 1018
2.0 × 10-37
5.0 × 1036
4.9 × 10-17
Question 5 (1 point)
Pure solids and liquids have constant concentration, regardless of total amount.
Question 5 options:
True
False
Question 6 (1 point)
A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products.
Question 6 options:
True
False
Question 7 (1 point)
When K << 1, the reverse reaction is favored
Question 7 options:
True
False
Question 8 (1 point)
When K >> 1, the forward reaction is favored
Question 8 options:
True
False
Question 9 (1 point)
If Q < K, it means the reverse reaction will proceed to form more reactants.
Question 9 options:
True
False
Question 10 (1 point)
The equilibrium constant does not change with changes in temperature.
Question 10 options:
True
False
Question 11 (1 point)
The equilibrium constant holds true for systems at equilibrium
Question 11 options:
True
False
Question 12 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?
Question 12 options:
1- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

2- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved


3- The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen
Question 13 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?
Question 13 options:
1- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.

2- The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.

3- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved

Question 14 (2 points)
Write the equilibrium expression for 2NO(g) + 2H2(g) N2(g) + 2H2O(g).
Question 14 options:
Kc = [NO]2 [H2]2 / [H2O]2 [N2]
Kc = [H2O]2 [N2] / [NO]2 [H2]2
Kc = [N2] / [NO]2 [H2]2
Question 15 (2 points)
The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?
Question 15 options:
Q = 5.15 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 15.2 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 0.194 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium

  
Question 1 (2 points)
Write the equilibrium expression for H2O(g) + CO(g) H2(g) + CO2(g)
Question 1 options:
1- Kc = [CO2] [H2] / [H2O] [CO]
2- Kc = [H2O] [CO] / [CO2] [H2]
3- Kc = [CO2] [H2] / [CO]
4- none

Question 2 (2 point)
What is n for the following equation in relating Kc to Kp?
N2(g) + 3 H2(g) 2 NH3(g)
Question 2 options:

2
4
-2
-4

Question 3 (3 points)
The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500 K?
N2(g) + 3 H2(g) 2 NH3(g)

Question 3 options:
61
3.6 × 10-2
1.9 × 10-2
15
28

Question 4 (3 points)
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.
2 N2(g) + O2(g) 2 N2O(g)

Question 4 options:
2.2 × 10-19
4.5 × 1018
2.0 × 10-37
5.0 × 1036
4.9 × 10-17
Question 5 (1 point)
Pure solids and liquids have constant concentration, regardless of total amount.
Question 5 options:
True
False
Question 6 (1 point)
A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products.
Question 6 options:
True
False
Question 7 (1 point)
When K << 1, the reverse reaction is favored
Question 7 options:
True
False
Question 8 (1 point)
When K >> 1, the forward reaction is favored
Question 8 options:
True
False
Question 9 (1 point)
If Q < K, it means the reverse reaction will proceed to form more reactants.
Question 9 options:
True
False
Question 10 (1 point)
The equilibrium constant does not change with changes in temperature.
Question 10 options:
True
False
Question 11 (1 point)
The equilibrium constant holds true for systems at equilibrium
Question 11 options:
True
False
Question 12 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?
Question 12 options:
1- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

2- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved


3- The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen
Question 13 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?
Question 13 options:
1- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.

2- The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.

3- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved

Question 14 (2 points)
Write the equilibrium expression for 2NO(g) + 2H2(g) N2(g) + 2H2O(g).
Question 14 options:
Kc = [NO]2 [H2]2 / [H2O]2 [N2]
Kc = [H2O]2 [N2] / [NO]2 [H2]2
Kc = [N2] / [NO]2 [H2]2
Question 15 (2 points)
The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?
Question 15 options:
Q = 5.15 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 15.2 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 0.194 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium

  
Question 1 (2 points)
Write the equilibrium expression for H2O(g) + CO(g) H2(g) + CO2(g)
Question 1 options:
1- Kc = [CO2] [H2] / [H2O] [CO]
2- Kc = [H2O] [CO] / [CO2] [H2]
3- Kc = [CO2] [H2] / [CO]
4- none

Question 2 (2 point)
What is n for the following equation in relating Kc to Kp?
N2(g) + 3 H2(g) 2 NH3(g)
Question 2 options:

2
4
-2
-4

Question 3 (3 points)
The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 500 K?
N2(g) + 3 H2(g) 2 NH3(g)

Question 3 options:
61
3.6 × 10-2
1.9 × 10-2
15
28

Question 4 (3 points)
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 × 10-18 M.
2 N2(g) + O2(g) 2 N2O(g)

Question 4 options:
2.2 × 10-19
4.5 × 1018
2.0 × 10-37
5.0 × 1036
4.9 × 10-17
Question 5 (1 point)
Pure solids and liquids have constant concentration, regardless of total amount.
Question 5 options:
True
False
Question 6 (1 point)
A reaction quotient (Q) larger than the equilibrium constant (K) means that the reaction will favor the production of more products.
Question 6 options:
True
False
Question 7 (1 point)
When K << 1, the reverse reaction is favored
Question 7 options:
True
False
Question 8 (1 point)
When K >> 1, the forward reaction is favored
Question 8 options:
True
False
Question 9 (1 point)
If Q < K, it means the reverse reaction will proceed to form more reactants.
Question 9 options:
True
False
Question 10 (1 point)
The equilibrium constant does not change with changes in temperature.
Question 10 options:
True
False
Question 11 (1 point)
The equilibrium constant holds true for systems at equilibrium
Question 11 options:
True
False
Question 12 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?
Question 12 options:
1- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

2- The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieved


3- The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen
Question 13 (2 points)
Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) H2(g) + CO2(g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?
Question 13 options:
1- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved.

2- The addition of carbon monoxide gas would not disrupt the equilibrium, so nothing would happen.

3- The addition of carbon monoxide gas would disrupt the equilibrium causing it to shift towards the right which would result in more products being produced until equilibrium is achieved

Question 14 (2 points)
Write the equilibrium expression for 2NO(g) + 2H2(g) N2(g) + 2H2O(g).
Question 14 options:
Kc = [NO]2 [H2]2 / [H2O]2 [N2]
Kc = [H2O]2 [N2] / [NO]2 [H2]2
Kc = [N2] / [NO]2 [H2]2
Question 15 (2 points)
The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?
Question 15 options:
Q = 5.15 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 15.2 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium
Q = 0.194 which is less than Kc, therefore the reaction needs to proceed towards the right to reach equilibrium

  

Explanation / Answer

For the given reaction , equilibrium constant = [H2] [CO2]/[H2O] [CO]

So option A is correct.

2. deltan= moles of products- moles of reactants= 2-3-1= -2 (C is correct)

3. Kp = KC*(RT) deltan = 61*(0.0821*500)-2 =0.0362 ( B is correct)

4. for the given reaction, Kc= [N2O]2/ [N2]2[O2] = (3.3*10-18)2/ 3.6*3.6*(4.1)

= 2*10-37   ( C is correct)

5. Concentration = moles/L. For pure solids and liquids, C= density/molar mass. For pure liquid or solids, density remains the same and hence constant concentration. True

6. Let us say for a reaction A<--->B, reaction coefficient Q= [B]/[A]. Since Q>K, more B is there and less A is there. Q>K suggests more of product B than A. True

7. for the reaction in 6, K= [B]/[A] when K<<1, more A and less B. Hence reactant favoured. True

8. For the same reason in 7, K>>1 more of B and less of A. Hence product favoured.

9. Q=K refers to equilibrium and Q>K, more of B than equilibrium B. Hence reaction shifts back wards. For Q<K, the reaction proceeds to the products. False

Question 10 (1 point)

10.As per Van;t Hoff equation, equilibrium constant is a function of temperature

Ln(K2/K1)= (deltaH/R)*(1/T1-1/T2) ( True)

11. True

12. KC = [H2][CO2]/[H2O][CO2]

Addition of H2 increases the numerator and to keep KC constant more of H2O and CO2 form. Hence shifts to the left. ( 1 is correct).

13. When CO is added, denominator decrease and to keep the equilibrium constant at the given value more products are formed and equilibrium shifts to right.

KC=[N2][H2O]2/ [H2]2 [NO]2    ( B is correct)

15. for the reaction H2+I2--à2HI

Q= [HI]2/[H2][I2] = 0.338*0.338/(0.112*0.198)= 5<K hence reaction proceeds towards product side to make Q larger. ( A is correct)

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