The value of K_c for the following reaction at 717 K is 48.

The value of Kc for the reaction
N₂O₂(g) \(\rightleftharpoons \) 2NO₂(g)

One mole of H₂ and one mole of I₂ are allowed to attain equilibrium in 1 lit container. If the equilibrium mixture contains 0.4 mole of HI. Calculate the equilibrium constant.

The equilibrium concentrations of NH₃, N₂ and H₂ are 1.8 x 10^-2 M, 1.2 x 10^-2 M and 3 x 10^-2 M respectively. Calculate the equilibrium constant for the formation of NH₃ from N₂ and H₂. [Hint: M= mol lit^-1]

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C

For the reaction,
A₂(g) + B₂(g) ⇌ 2AB(g) ; ΔH is –ve.
the following molecular scenes represent different reaction mixture (A – green, B – blue)

i) Calculate the equilibrium constant K_P and (K_C).
ii) For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
iii) What is the effect of increase in pressure for the mixture at equilibrium.

One mole of PCl₅ is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.

For the reaction
SrCO₃ (s) ⇌ SrO (s) + CO₂(g),
the value of equilibrium constant K_P = 2.2 x 10^–4 at 1002 K. Calculate K_C for the reaction.

To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500^o C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate K_C and K_{P for this reaction.}

Oxidation of nitrogen monoxide was studied at 200^o C with initial pressures of 1 atm NO and 1 atm of O₂. At equilibrium partial pressure of oxygen is found to be 0.52 atm calculate K_P value.