Question

Consider the following system at equilibrium where H° = 111 kJ, and K_c = 6.30, at 723 K.

2NH₃(g) N₂(g) +  3H₂(g)  

When 0.22 moles of N₂(g) are added to the equilibrium system at constant temperature:

please double check answer to make sure its correct, thank you.

The value of K_c _________increases.decreases.remains the same.

The value of Q_c  _________is greater than is equal to is less than K_c.

The reaction must ?

run in the forward direction to restablish equilibrium.
run in the reverse direction to restablish equilibrium.
remain the same. It is already at equilibrium.

The concentration of H₂ will _increase/decrease/remain the same________increase.decrease.remain the same.

Answer 1

1. The value of Kc remains the same.

Explanation: Equilibrium constant is independent of concentration but depends on temperature. When 0.22 moles of N2(g) are added to the equilibrium system at constant temperature, Equilibrium constant remains the same.

2. Equal

Explanation: At equilibrium the value of Qc is equal to Kc.

3. Must run in the reverse direction to restablish equilibrium.

Explanation: According to Le Chatelier's principle increase in concentration of products will run the reaction in backwards.

4. The concentration of H2 will decrease.

Explanation: Since N2 is increased, H2 will decrease to attain equilibrium.