Chemical Equilibrium - Physical Chemistry - Chemistry Previous Year Questions

For the formation of ammonia gas from its constituent elements, the $K_p / K_C$ is

At 780 K and 10 atmosphere pressure the equilibrium constant for the reaction $2 A(g) \rightleftharpoons B(g)+C(g)$ is 3.52 . At the same temperature and 7.04 atmosphere pressure, the equilibrium constant for the same reaction is

229, $\mathrm{At} T(\mathrm{~K}), K_C$ value for the reaction, $\frac{1}{3} \mathrm{~N}_2(g)+\mathrm{H}_2(g) \rightleftharpoons \frac{2}{3} \mathrm{NH}_3(g)$ is 50 . The $K_C$ value for the reaction, $2 \mathrm{NH}_3(g) \rightleftharpoons \mathrm{N}_2(g)+3 \mathrm{H}_2(g)$ at the same temperature is

At $T(\mathrm{~K})$ when one mol of $X$ and one mol of $Y$ are heated in a 1 L flask, 0.5 moles of $Z$ is formed at the equilibrium. The $K_C$ value of the reaction is

$$X(g)+Y(g) \rightleftharpoons Z(g)+A(g)$$

The vapour density of $\mathrm{N}_2 \mathrm{O}_4$ in $\mathrm{N}_2 \mathrm{O}_4 \rightleftharpoons 2 \mathrm{NO}_2$ is 40 . The degree of dissociation is

What is the equilibrium constant $\left(K_C\right)$ for the given reaction?

$$\mathrm{N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO}$$

Where the equilibrium concentration of $\mathrm{N}_2, \mathrm{O}_2$ and NO are found to be $4 \times 10^{-3}, 3 \times 10^{-3}$ and $3 \times 10^{-3} \mathrm{M}$ respectively.

The $K_p$ value at equilibrium of $\mathrm{SO}_3$ formation reaction from $\mathrm{SO}_2(g)$ and $\mathrm{O}_2(g)$ is $5 \mathrm{~atm}^{-1}$. What is the equilibrium partial pressure of $\mathrm{O}_2$ if the equilibrium pressure of $\mathrm{SO}_2$ and $\mathrm{SO}_3$ are equal?

In which of the following reactions at equilibria, the position of the equilibrium shifts towards the products, if the total pressure is increased?

(i) $X_2(g)+3 Y_2(g) \rightleftharpoons 2 X_3(g)$

(ii) $X_2(g)+Y_2(g) \rightleftharpoons 2 X Y(g)$

(iii) $X_2(g)+Z_2(g) \rightleftharpoons 2 X Z(g)$

(iv) $X_2(g)+Y_4(g) \rightleftharpoons 2 X Y_2(g)$

Calculate the value of the equilibrium constant $\left(K_p\right)$ for the reaction of oxygen gas oxidising ammonia gas to nitric oxide and water vapour. The pressure of each gas at equilibrium is 0.5 atm .

For the formation of ammonia from its constituent elements ( 1 mole of $\mathrm{N}_2$ and 3 moles of $\mathrm{H}_2$ ) in a closed vessel of volume $V(\mathrm{~L})$, the value of $K_C$ is [units of $K_C=\mathrm{mol}^{-2} \mathrm{~L}^2$ ]

Aqueous solution of ferric nitrate when mixed with aqueous solution of potassium thiocyanate gives red colour solution. The intensity of red colour becomes constant on attaining equilibrium.

Choose the correct statement when the following chemical is added to the above solution at equilibrium.

I. Oxalic acid

II. Mercuric chloride

For the given equilibrium reaction

$$\mathrm{H}_2(\mathrm{~g})+\mathrm{I}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{~g})$$

Choose the correct equation to calculate $K_p$.

For a given equilibrium reaction, addition of inert argon gas at constant volume can shift the equilibrium in

$$\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \rightleftharpoons 2 \mathrm{NH}_3(g)$$

For a reversible reaction $A \rightleftharpoons B$, pre-exponential factor is same for both the forward and backward reactions and has value of $20 \mathrm{~S}^{-1}$. If the enthalpy change along the forward reaction is $-41.5 \mathrm{~kJ} / \mathrm{mol}$, the value of equilibrium constant at 500 K is

For a given reaction, $2 A \rightleftharpoons B+C$, the equilibrium constant is $2 \times 10^{-3}$. If at any given time the composition of the reaction mixture is $[A]=[B]=[C]=6 \times 10^{-5} \mathrm{M}$; predict in which direction the reaction will proceed and the correct value for reaction quotient.