The equilibrium constant (K_C) for the reaction N₂(g) + O₂(g) $$\to$$ 2NO(g) at temperature T is 4 $$\times$$ 10^–4. The value of K_C for the reaction, NO(g) $$\to$$ 1/2N₂(g) + 1/2O₂(g) at the same temperature is :

A vessel at 1000 K contains CO₂ with a pressure of 0.5 atm. Some of the CO₂ is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is :

In aqueous solution the ionization constants for carbonic acid are
K₁ = 4.2 x 10^–7 and K₂ = 4.8 x 10^–11
Select the correct statement for a saturated 0.034 M solution of the carbonic acid.

The equilibrium constants K_P1 and K_P2 for the reactions X $$\leftrightharpoons$$ 2Y and Z $$\leftrightharpoons$$ P + Q, respectively are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal then the ratio of total pressure at these equilibria is :