Question

Consider the following system at equilibrium where AH° = -111 kJ, and K = 0.159, at 723 K N2(g) +3H2(g)=2NH3(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of K A. increases B. decreases. C. remains the same. The value of Qc A. is greater than K B. is equal to Ke. C. is less than K A. run in the forward direction to reestablish equilibrium The reaction must: B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of H2 will: A. increase. B. decrease. C. remain the same.

Answer 1

Answer :-

For a equilibrium reaction, if the volume in increased, the reaction will proceed in the direction in which there is more gaseous molecules. So for the given reaction, the gaseous molecules are on the backward direction i.e left side.

So, The value of Kc = C. remains the same.

The value of Qc = A. Is greater than Kc

The reaction must = B. run in the reverse direction

The number of moles of H₂ will := A. increase