In a 0.5 litre capacity vessel, CO and Cl₂ are mixed to form COCl₂. At equilibrium, it contains 0.2 mole of COCl₂ and 0.1 mole each of CO and Cl₂. The equilibrium constant (K_c) for the following reaction is: \(CO + Cl_2 ⇌ COCl_2\)

1.	15	2.	5
3.	20	4.	10

Find K_c for the equilibrium:

2H₂S(g) ⇌ 2H₂(g) + S₂(g)

An equilibrium mixture contains 1.0 mol H₂S, 0.2 mol H₂, and 0.8 mol S₂ in a 2.0 L flask.

1. 0.08

2. 0.016

3. 0.004

4. 0.160

1.25 moles of NOCl were placed in a 2.50 L reaction chamber at $427°\mathrm{C}.$ After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant K_c for the reaction,

$2\mathrm{NOCl}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

1. $1.6\times {10}^{-3}$

2. $5.6\times {10}^{-4}$

3. $2.6\times {10}^{-3}$

4. $4.6\times {10}^{-4}$

Find the acid dissociation constant (Kₐ) of HXO given that:

XO⁻(aq) + H₂O(l) ⇌ HXO(aq) + OH⁻(aq)

K = 0.36 × 10⁻⁶

The equilibrium constant value for the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>1.48\times {10}^{-5}$, the value for the reaction $1/2{\mathrm{N}}_2\left(\mathrm{g}\right)+3/2{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>\mathrm{n}\times {10}^{-3}$ where n is

1. 1.85

2. 3.85

3. 4.85

4. 10

A gaseous phase reaction is allowed to attain equilibrium as $\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right)$ at constant pressure P. The partial pressure of A at equilibrium is P/2. The value of equilibrium constant K_p is

1. $\frac{\mathrm{P}}{8}$

2. $\frac{\mathrm{P}}{6}$

3. $\frac{\mathrm{P}}{2}$

4. $\frac{\mathrm{P}}{4}$

Two moles of N₂O₄ is heated to form NO and O₂. As soon as NO and O₂ are formed they react to form N₂O₅. Two equilibria

${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2\mathrm{NO}+{\mathrm{O}}_2$
$2\mathrm{NO}+\frac{3}{2}{\mathrm{O}}_2\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_5$

Are simultaneously established. At equilibrium, the degree of dissociation of N₂O₄ was found to 50%. Which of the following is correct at equilibrium?

1. $\frac{1}{2}\left[\mathrm{NO}\right]=\frac{3}{2}\left[{\mathrm{O}}_2\right]$

2. $2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]=\left[\mathrm{NO}\right]+\frac{3}{2}\left[{\mathrm{O}}_2\right]+\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]$

3. $\left[\mathrm{NO}\right]+\left[{\mathrm{O}}_2\right]=\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]+\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]$

4. $\frac{1}{2}\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]+\left[{\mathrm{O}}_2\right]=\frac{1}{2}\left[\mathrm{NO}\right]$

Find Kₚ for the following equilibrium at 25°C:

NH₄HS(s) ⇌ NH₃(g) + H₂S(g)

The total equilibrium pressure is 0.660 atm.

1. 0.109

2. 0.218

3. 1.89

4. 2.18

PCl₅ is 50% dissociated at $20°\mathrm{C}$ and 1 atm pressure. The value of K_p for this reaction is:

Find the equilibrium concentrations of SO₂ and SO₃ for the reaction:

SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Given Kc = 16. Initially, 1 mol each of SO₂, NO₂, SO₃ and NO is taken in a 1 L vessel.

1. 0.4, 0.8

2. 0.8, 0.16

3. 1.6, 0.8

4. 0.4, 1.6