Chemical Equilibrium - Physical Chemistry - Chemistry Previous Year Questions

\(2S{O_2}(g) + {O_2}(g)\buildrel {{V_2}{O_5}} \over \[\rightleftharpoons\) is an example for\]

In the chemical reaction,

N\(_2\) + 3H\(_2\) \(\rightleftharpoons\) 2NH\(_3\) at equilibrium point.

For the equilibrium,

2NOCl(g) \(\rightleftharpoons\) 2NO(g) + Cl\(_2\)(g),

the value of the equilibrium constant, \(K_C\) is 3.75 \(\times\) 10\(^{-6}\) at 1069 K. The value of \(K_p\) for the reaction at this temperature will be

In the equilibrium, \(AB\rightleftharpoons A+B\), if the equilibrium concentration of A is double, then equilibrium concentration of B will be

For the reaction, H\(_2\)(g) + I\(_2\)(g) \(\rightleftharpoons\) 2HI(g) the position of equilibrium can be shifted to the right by

The equilibrium constant, \(K_C\) for \(3C_2H_2(g) \rightleftharpoons C_6H_6(g)\) is 4 L\(^2\)mol\(^{-2}\). If the equilibrium concentration of benzene is 0.5 mol\(^{-1}\) than what is the value of concentration of ethylene?

The equilibrium constants for the reactions \(a, b\), and \(c\) are as given:

a) \(\mathrm{N}_2+3 \mathrm{H}_2=2 \mathrm{NH}_3: \mathbf{K}_1\)

b) \(\mathrm{N}_2+\mathrm{O}_2=2 \mathrm{NO}: \mathrm{K}_2\)

c) \(2 \mathrm{H}_2+\mathrm{O}_2=2 \mathrm{H}_2 \mathrm{O}: \mathbf{K}_3\)

What would be the Equilibrium constant for the reaction:

$$4 \mathrm{NH}_3+5 \mathrm{O}_2=4 \mathrm{NO}+6 \mathrm{H}_2 \mathrm{O} ; \mathbf{K}_{\mathbf{x}}$$

\(\mathrm{S}_8\) on heating at a temperature above \(1000 \mathrm{~K}\), changes to \(\mathrm{S}_2\). When 1 mole of \(\mathrm{S}_8\) is heated above \(1000 \mathrm{~K}\), the pressure falls by \(32 \%\) at equilibrium. The equilibrium constant for the conversion is:

At \(700 \mathrm{~K}\), the Equilibrium constant value for the formation of \(\mathrm{HI}\) from \(\mathrm{H}_2\) and \(\mathrm{I}_2\) is 49.0 . 0.7 mole of \(\mathrm{HI}(\mathrm{g})\) is present at equilibrium. What will be the concentrations of \(\mathrm{H}_2\) and \(\mathrm{I}_2\) gases if we initially started with \(\mathrm{HI}(\mathrm{g})\) and allowed the reaction to reach equilibrium at the same temperature?

Consider the reaction

$$\mathrm{Fe}_2 \mathrm{O}_3(\mathrm{~s})+3 \mathrm{CO}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{Fe}(\mathrm{l})+3 \mathrm{CQ}_2(\mathrm{~g})$$

In accordance with Le-Chatlier's principle, which of the following will not disturbs the equilibrium?

For a reaction,

$$A+B \rightleftharpoons 2 C$$

1.0 mole of $A, 1.5$ mole of $B$ and 0.5 mole of $C$ were taken in a 1 L vessel. At equilibrium, the concentration of $C$ was $1.0 \mathrm{~mol} \mathrm{~L}^{-1}$. The equilibrium constant for the reaction is $x / 15$. The value of ' $x$ ' is:

Consider the following equilibrium,

$$\begin{aligned} & 2 \mathrm{No}(g) \rightleftharpoons \mathrm{N}_2+\mathrm{O}_2 ; \mathrm{K}_{\mathrm{G}}=2.4 \times 10^{20} \\ & \mathrm{No}(\mathrm{g})+\frac{1}{2} \mathrm{Br}_2(\mathrm{~g}) \rightleftharpoons \mathrm{NoBr}(\mathrm{g}) ; \mathrm{K}_{\mathrm{C}_2}=1.4 \end{aligned}$$

Calculate \(K_C\) for the reaction,

$$\frac{1}{2} \mathrm{~N}_2(g)+\frac{1}{2} \mathrm{O}_2(g)+\frac{1}{2} \mathrm{Br}_2(g) \rightleftharpoons \mathrm{NOBr}(g)$$

If the equilibrium constant for $\mathrm{N}_{2(g)}+\mathrm{O}_{2(g)} \rightleftharpoons 2 \mathrm{NO}_{(g)}$ is 49 The equilibrium constant for the reaction $N O_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)}+\frac{1}{2} O_{2(g)}$ is $\_\_\_\_$

Consider the gaseous equilibrium

$2 \mathrm{AB}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{AB}_{(\mathrm{g})}+\mathrm{B}_{2(\mathrm{~g})}$

The expression relating the degree of dissociation ( $\alpha$ ) and equilibrium constant ( $K_p$ ) and total pressure $P$ is:

An equilibrium mixture taken in 2 litre vessel of the reaction: $2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{SO}_3(\mathrm{~g})$ has 4 moles of $\mathrm{SO}_2, 3$ moles of $\mathrm{O}_2$ and 6 moles of $\mathrm{SO}_3$ then the value of equilibrium constant $\left(\mathrm{K}_c\right)$ will be: