Question

Consider the following system at equilibrium where AH° = 16.1 kJ, and K. -6.50x103, at 298 K: 2NOBr(g) 22NO(g) + Brz(8) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of KC A. Increases B. Decreases C. Remains the same The value of QC A. Is greater than K B. Is equal to K C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase B. Decrease. C. Remain the same.

Answer 1

1. With the increase in temperature the value of Kc decreases. Acc. to Le Chatelier's Principle with the increase in temperature the move the reaction to the left. It is done because equillibrium shift in such a way to reduce the temperature again.

2. Is greater then Kc.

As the reaction is shifting to the left side due to increase in temperature , the shifting of reaction to the left occurs when Qc > Kc.

3. Run im the reverse direction to restablish the equillibrium.

4. Concentration of Br2 will decrease , as the reaction is moving to the left direction.

Hopefully it will help you.

Thank you.