At 500 K, equilibrium constant, K_c , for the following reaction is 5.

$\frac{1}{2}{\mathbf{H}}_2$ (g) + $\frac{1}{2}{\mathbf{I}}_2$  (g) ⇌ HI (g)

What would be the equilibrium constant K_c for the reaction

2HI(g) ⇌ H₂ (g) + I₂ (g)

(i) 04

(ii) 4

(iii) 25

(iv) 5

pH for 0.01 M NaOH solution is

K_p for the given reaction is (36 × 10^–2atm^–1) Find out K_c (M^–1) (nearest integer).

(2NO₂ N₂O₄)

(R=0.0821 atm. L/mol. K)

(T = 300K)

A(g) ->B(g) + $\frac{1}{2}$ <!-- [if gte mso 9]><xml> </xml><![endif]-->C(g)

In the about reaction, the correct relation between K_p, a and equilibrium pressure (p) is

Which of the following equilibrium will shift in forward direction on applying pressure?

The ionization constant of HCN is 4.5 × 10^–10 at 298 K. Hydrolysis constant of sodium cyanide is