Chemical Equilibrium · Chemistry · TS EAMCET

At $T(\mathrm{~K}), K_p$ value for the reaction,

$$ 2 \mathrm{AO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AO}_3(\mathrm{~g}) \text { is } 4 \times 10^{10}, $$

What is the $K_p^{\prime}$ value for

$$ 2 \mathrm{AO}_2(\mathrm{~g})+\frac{3}{2} \mathrm{O}_2 \rightleftharpoons 3 \mathrm{AO}_3(\mathrm{~g}) \text { at } T(\mathrm{~K}) $$

At 1000 K , the equilibrium constant for the reaction, $\mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$ is 0.53 . In a one litre vessel, at equilibrium the mixture contains 0.25 mole of $\mathrm{CO}, 0.5$ mole of $\mathrm{CO}_2, 0.6$ mole of $\mathrm{H}_2$ and $x$ moles of $\mathrm{H}_2 \mathrm{O}$. The value of $x$ is

For the reaction $\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g)$, the correct relation between degree of dissociation $(\alpha)$ of $\mathrm{N}_2 \mathrm{O}_4(g)$ and equilibrium constant, $K_p$ is ( $p=$ total pressure of mixture)

At $T(K)$ the equilibrium constants for the following two reactions are given below

$ 2 A(g) \rightleftharpoons B(g)+C(g) ; K_{1}=16 $

$ 2 B(g)+C(g) \rightleftharpoons 2 D(g) ; K_{2}=25 $

What is the value of equilibrium constant $(K)$ for the reaction given below at $T(K)$ ?

$ A(g)+\frac{1}{2} B(g) \rightleftharpoons D(g) $

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

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

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

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 $K_C=\mathrm{mol}^{-2} \mathrm{~L}^2$ ]

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

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

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 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 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 $K_p$.

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

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.