Consider the following system at equilibrium where 11104 kJ

Consider the following system at equilibrium where 11°-10.4 kJ, and Kc = 1.80x10-2, at 698 K. 2H1(g) =-H2(g) + 12(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Kc A. increases. B. decreases. C. remains the same. The value of Qe A. is greater than Ke is equal to Kc B. is equal to Kc C. is less than Kc A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The reaction must: The number of moles of 12 will:A. increase. B. decrease. C. remain the same

Solution

Volume is increased , so the pressure will be reduced.

Since the reaction has same pressure ( due to equal number of moles of gas) on both the sides , :

The value of Kc remains the same.

The value of Kc is equal to Kc

The reaction must remain the same . It is already at equillibrium.

The number of moles of I2 remain the same.