In the following questions two or more options may be correct.

For the reaction N₂O₄ (g) ⇌2NO₂ (g), the value of K is 50 at 400 K and 1700 at 500 K. Which of the following options is correct?

(i) The reaction is endothermic

(ii) The reaction is exothermic

(iii) If NO₂ (g) and N₂O₄ (g) are mixed at 400 K at partial pressures 20 bar and 2 bar respectively, more N₂O₄ (g) will be formed.

(iv) The entropy of the system increases.

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