Following data is given for the reaction: CaCO₃ (s) → CaO (s) + CO₂ (g)

 ∆_fHᶱ [CaO(s)] = – 635.1 kJ mol^–1

 ∆_fHᶱ[CO₂(g)] = – 393.5 kJ mol^–1

∆_fHᶱ[CaCO₃(s)] = – 1206.9 kJ mol^–1

Predict the effect of temperature on the equilibrium constant of the above reaction.

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