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- 1. Multiple Choice
Which of the following is true about chemical reaction at equilibrium
only the forward reaction stops
only the reverse reaction stops
both forward and reverse reactions stop
the rate constants for the forward and reverse reactions are equal
the rates of the forward and reverse reactions are equal
- 2. Multiple Choice
How is the reaction quotient used to determine whether a system is at equilibrium?
At equilibrium, the reaction quotient is undefined.
The reaction is at equilibrium when Q < K.
The reaction is at equilibrium when Q > K.
The reaction is at equilibrium when Q = K.
- 3. Multiple Choice
If the reaction quotient Q has a smaller value than the related equilibrium constant, K, _________
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of the reactants
the reaction is not at equilibrium, and will make more reactants at the expense of the products
the value of K will not increase until it is equal to Q
- 4. Multiple Choice
If the reaction quotient Q has a value larger than the related equilibrium constant, K _________
the reaction is at equilibrium
the reaction is not at equilibrium, and will make more products at the expense of reactants
the reaction is not at equilibrium, and will make more reactants at the expense of products
the value of K will increase until it is equal to Q
- 5. Multiple Choice
The value of the equilibrium constant, Kp for the reaction below is 3.1 × 10-4 at 700K.
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
Given the initial partial pressure of the gases, PN2 = 0.411 atm; PH2 = 0.903 atm; PNH3 = 0.224 atm, calculate the value of the reaction quotient, Q.
Q = 0.0437
Q = 0.1658
Q = 0.6036
Q = 0.1352
- 6. Multiple Choice
The value of the equilibrium constant, Kp for the reaction below is 3.1 × 10-4 at 700K.
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
Given the initial partial pressure of the gases, PN2 = 0.411 atm; PH2 = 0.903 atm; PNH3 = 0.224 atm. Predict the direction in which the reaction will proceed at 700 K.
Since Q > Kp, the equilibrium will proceed to the left to bring the value Q down to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the right to bring the value Q down to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the left to bring the value Q up to 3.1 × 10-4.
Since Q > Kp, the equilibrium will proceed to the right to bring the value Q up to 3.1 × 10-4.
- 7. Multiple Choice
For the reaction system:
2HI (g) ↔ H2 (g) + I2 (g)
Kc = 0.020 at 720 K
If the initial concentrations of HI, H2 and I2 are all 1.50 × 10-3 M at 720 K, which one of the following statements is correct?
The system is at equilibrium.
The concentrations of HI and I2 will increase as the system is approaching equilibrium.
The concentration of HI will increase as the system is approaching equilibrium.
The concentration of H2 and I2 will increase as the system is approaching equilibrium.
- 8. Multiple Choice
For the reaction, N2O4 (g) ↔ 2NO2 (g), Kc = 0.21 at 100oC. At initial, the [N2O4] = 0.12 M and [NO2] = 0.55 M. Is the reaction at equilibrium? If not, in which direction it is progressing?
Yes, the reaction is at equilibrium.
No, the reaction is not at equilibrium. Qc < Kc, therefore the reaction will proceed from left to right until Qc = Kc.
No, the reaction is not at equilibrium. Qc > Kc, therefore the reaction will proceed from right to left until Qc = Kc.
No, the reaction is not at equilibrium. Qc < Kc, therefore the reaction will proceed from right to left until Qc = Kc.
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