7.24. Calculate (a) ∆G^ϴ and (b) the equilibrium constant for the formation of NO₂ from NO and O₂ at 298 K

NO (g) + ½ O₂ (g)​⇌ NO₂ (g)

where

Δ_fG^ϴ (NO2) = 52.0 kJ/mol

Δ_fG^ϴ (NO) = 87.0 kJ/mol

Δ_fG^ϴ (O2) = 0 kJ/mol  

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