Chemical Equilibrium Questions

For N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat –

For the reaction : N₂O₃(g) ⇌ NO(g) + NO₂(g) ; total pressure = P, degree of dissociation = 50%. Then Kₚ would be –

For the reaction A(g) + B(g) ⇌ C(g) + D(g), the degree of dissociation α would be –

At 444° C, the equilibrium constant K for the reaction 2AB(g) ⇌ A₂(g) + B₂(g) is 1/64. The degree of dissociation of AB will be -

The equilibrium concentration of X, Y and YX₂ are 4, 2 and 2 mole L⁻¹ respectively for the equilibrium 2X(g) + Y(g) ⇌ YX₂(g). The value of Kc is -

If in the reaction N₂O₄(g) ⇌ 2NO₂(g), α is the part of N₂O₄ which dissociates then the number of moles at equilibrium will be -

For the reaction, 2NO₂(g) ⇌ 2NO(g) + O₂(g), Kc = 1.8 × 10⁻⁶ at 185°C. At 185°C, the value of Kc for the reaction - NO(g) + ½ O₂(g) ⇌ NO₂(g) is -

The reaction A(g) + B(g) ⇌ C(g) + D(g) proceeds to right hand side upto 99.9%. The equilibrium constant K for the reaction will be -

The equilibrium constant Kc for the decomposition of PCl₅ is 0.625 mole / lit at 300°C. Then the value of Kₚ is -

Select the correct expression regarding the relation between Kₚ and Kc for the reaction aX(g) + bY(g) ⇌ bZ(g) + aW(g) -

In which of the following reaction, the value of Kₚ will be equal to Kc –

The value of Kₚ for the reaction H₂(g) + I₂(g) ⇌ 2HI(g) is 50. What is the value of Kc

K₁ and K₂ are the rate constants of forward and backward reactions. The equilibrium constant K of the reaction is -

In a chemical equilibrium, the equilibrium constant is found to be 2.5. If the rate constant of backward reaction is 3.2 × 10⁻², the rate constant of forward reaction is -

According to Law of Mass action, the rate of reaction is directly proportional to -

A chemical reaction A ⇌ B is said to be in equilibrium when -

At any moment before a reversible reaction attains equilibrium it is found that –

Which of the following statements is false in case of equilibrium state –

Chemical equilibrium is dynamic in nature because –

For the reaction A(g) + 3B (g) →2C (g) at 27°C, 2 moles of A, 4 moles of B and 6 moles of C are present in 2 litre vessel. If KC for the reaction is 1.2, the reaction will proceed in :

At temperature, T, a compound AB2(g) dissociates according to the reaction; 2AB2(g) → 2AB(g) + B2(g) with a degree of dissociation x, which is small compared with unity. The expression for Kp, in terms of x and the total pressure, P is

For the reaction N2 + 3H2 →2NH3 , N2 & H2 were taken in the molar ratio of 1 : 3 . Up to the point of equilibrium 50% each reactant has been reacted. If total pressure at equilibrium is P. The partial pressure of ammonia would be

The value of KC for the reaction :A + 3B → 2C is 0.5 at 400°C. Calculate the value of KP

At 27°C, it was observed in the hydrogenation reaction, the pressure of H2 gas decreases from 10 atm to 2 atm in 10 mins. Calculate the rate of reaction in M min−1.(Given: R = 0.08 lit atm K-1 mol-1 )

In the system, LaCl3(s) + H2O(g) + heat ⇌ LaClO(s) + 2HCl(g), equilibrium is established. More water vapour is added to reestablish the equilibrium. The pressure of water vapour is doubled. The factor by which pressure of HCl is changed is:

Mechanism of a hypothetical reaction X2 + Y2 → 2XY is given below :- (i) X2 ⇌ X + X (fast) (ii) X + Y2 → XY + Y (slow) (iii) X + Y → XY (fast) The overall order of the reaction will be :-