In the reaction ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$ at equilibrium, some I₂ is added. What happens to the equilibrium?

1. It gets shifted to the right

2. It remains unchanged

3. It gets shifted to the left

4. First 2 then 3

Which of the following reaction will be favoured at low pressure?

1. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$

2. ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$

3. ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$

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

For the reaction

${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

the forward reaction at constant temperature is favoured by

A. introducing an inert gas at constant volume

B. introducing chlorine gas at constant volume

C. introducing an inert gas at constant pressure

D. increasing the volume of the container

E. introducing PCl₅ at constant volume

1. A, B, C

2. D, E, C

3. B, C, E

4. A, D, E

For the reaction

$\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

at a given temperature, the equilibrium amount of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ can be increased by

1. Adding a suitable catalyst

2. Adding an inert gas

3. Decreasing the volume of the container

4. Increasing the amount of CO (g)

Which of the following cases leads to the reaction remaining fastest to completion?

1. $\mathrm{K}=1$

2. $\mathrm{K}=10$

3. $\mathrm{K}={10}^{-2}$

4. $\mathrm{K}={10}^2$

Consider the following reactions:

A. ${\mathrm{AB}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{AB}}_3\left(\mathrm{g}\right)$

B. $2{\mathrm{AB}}_3\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{AB}}_2+{\mathrm{B}}_2\left(\mathrm{g}\right)$

If K₁ and K₂ are the equilibrium constants at $27°\mathrm{C}$ in reactions A and B respectively, then K₁, and K₂ are related as

1. ${\mathrm{K}}_1^2={\mathrm{K}}_2$

2. ${\mathrm{K}}_2{\mathrm{K}}_1^2=1$

3. ${\mathrm{K}}_1=2{\mathrm{K}}_2$

4. ${\mathrm{K}}_1{\mathrm{K}}_2^2=1$

For the reaction, ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$, the equilibrium concentrations of H₂, I₂ and HI are 8, 3 and 28 mol L^-1 respectively. Equilibrium constant of the reaction is

1. 32.67

2. 31.67

3. 34.67

4. 36.67

In which of the following case, the value of K_p is less than K_c?

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

2. ${\mathrm{H}}_2+{\mathrm{Cl}}_2\rightleftharpoons 2\mathrm{HCl}$

3. $2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$

4. ${\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$

Equilibrium constants K₁, and K₂ for the following equilibria

$\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\stackrel{{\mathrm{K}}_1}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right) \mathrm{and}$
$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2$

are related as

1. ${\mathrm{K}}_2=1/{\mathrm{K}}_1^2$

2. ${\mathrm{K}}_2={\mathrm{K}}_1^2$

3. ${\mathrm{K}}_2=1/{\mathrm{K}}_1$

4. ${\mathrm{K}}_2={\mathrm{K}}_1/2$

In a chemical equilibrium rate constant of forward reaction is $7.5\times {10}^{-4}$ and the equilibrium constant is 1.5. The rate constant of a backward reaction is

1. $2.5\times {10}^4$

2. $5\times {10}^{-4}$

3. $2.5\times {10}^{-4}$

4. $5\times {10}^4$