Test: Chemical Equilibrium - 2 - Chemistry MCQ

The plot given below shows the relation between (1/T) and log(s), where S is the solubility of an electrolyte AB and T is the temperature in Kelvin. What conclusion can be drawn from the plot:

A mixture of 2 mole each of helium and an unknown gas (normal boiling point = 0°C) is kept in a 22.4 L flask. If the flask is cooled to 0.1°C, the resultant pressure (in atm) inside the flask is:           

For the complete oxidation of 100 g of Cyclohexanol to cyclohexanon, the quantity of CrO₃ required is (assuming 100% chemical yield) [Atomic wt. of Cr = 52)           

For the reaction: the equilibrium constant at 2000 K and 1.0 bar is 5.25. When the pressure is increased by 8-fold, the equilibrium constant:           

In a chemical reaction, 

The total pressure at equilibrium is 6 atm. The value of equilibrium constant is:

If the equilibrium constants for the reactions 1 and 2

Are K₁ and K₂, the equilibrium constant for the reaction

Consider the reaction, at equilibrium,

 The equilibrium can be shifted towards the forward direction by:

When a reversible reaction  is followed with time with initial concentration of A being 0.6 mol. L^–1, the following graph is obtained:

The equilibrium constant K, for the above reaction is:

If the equilibrium reaction  is heated, it is observed that the concentration of A increases. Then,

Consider the reaction:

The unit of the thermodynamic equilibrium constant for the reaction is:

For the reaction H₂(g)+I₂(g)⇌2HI (g) at 721 K
value of equilibrium constant is 50, when molar concentration of both hydrogen and iodine is 0.5 M at equilibrium value of Kp under the same conditions will be

A 2 L vessel containing 2g of H₂ gas at 27°C is connected to a 2L vessel containing 176 g of CO₂ gas at 27°C. Assuming ideal behaviour of H₂ and CO₂, the partial pressure of H₂ at equilibrium is………bar.

The relationship between the equilibrium constant K₁ for the reaction

And the equilibrium constant K₂ for the reaction

The hydrolysis constant (K_h) of NH₄Cl is 5.6×10^–10. The concentration of H₃O⁺ in a 0.1 M solution of NH₄Cl at equilibrium is:

The equilibrium constant K_c for the following reaction at 842°C is 7.90 × 10^–3. What is K_p at same temperature:

For the equilibrium what is the temperature at which

The pH of a solution of hydrochloric acid is 4. The molarity of the solution is:

Consider the following gaseous equilibria given below

The equilibrium constant for the reaction, in terms of K₁, K₂ and K₃ will be

9.2 grams of N₂O₄(g) is taken in a closed on litre vessel and heated till the following equilibrium is reached

At equilibrium, 50% N₂O₄(g) is dissociated. What is the equilibrium constant (in mol litre^–1) (molecular weight of N₂O₄ = 92)

In a chemical reaction: xenon gas is added at constant volume. The equilibrium:

The equilibrium constants for the reactions   and   are K₁ and K₂, respectively. The equilibrium constant for the reaction  is

Correct statement on the effect of addition of aq. HCl on the equilibrium is: