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

Find the changes that favour the forward reaction for the equilibrium:

PCl₅(g) ⇌ PCl₃(g) + Cl₂(g)

A. Addition of inert gas at constant volume
B. Addition of Cl₂ at constant volume
C. Addition of inert gas at constant pressure
D. Increase in volume of the container
E. Addition of PCl₅ at constant volume

1. A, B, C

2.  C, D, E

3. B, C, E

4. A, D, E

Find the change that increases the equilibrium amount of CO₂(g) for the reaction:

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)

at a constant temperature.

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 H₂ + I₂ ⇌ 2HI,
the equilibrium concentrations of hydrogen, iodine, and hydrogen iodide are
8 mol L⁻¹, 3 mol L⁻¹, and 28 mol L⁻¹ respectively.
What is the equilibrium constant (K_c) for this reaction?

1. 32.67
2. 28.67
3. 34.67
4. 38.67

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

$\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\stackrel{{\mathrm{K}}_1}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{and}$
$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2$

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. $5\times {10}^4$