The value of `K_c` for `2HF(g) = H_2(g) + F_2(g)` is `1.0 xx 10^(-3)` at a particular temperature. At a certain time, the concentrations of `HF, H_2` and `F_2` were found to be 0.5, `1xx10^(- 3)` and `4 xx 10^(-3)` mole/litre respectively. Is the reaction at equilibrium? If not, what would be the direction to attain equilibrium?

Explanation

To determine whether the reaction \(2HF(g) \rightleftharpoons H_2(g) + F_2(g)\) is at equilibrium, we need to compare the reaction quotient \(Q\) with the equilibrium constant \(K_c\).

### Step 1: Write the expression for \(K_c\)

The equilibrium constant expression for the reaction is given by:

\[
K_c = \frac{[H_2][F_2]}{[HF]^2}
...