An equilibrium mixture for the reaction,

$2{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_2\left(\mathrm{g}\right)$

had 1 mole of H₂S, 0.2 mole of H₂ and 0.8 mole of S₂ in a 2 litre flask. The value of K_c in mol L^-1 is

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. $4.6\times {10}^{-4}$

If equilibrium constant for the reaction,

${\mathrm{XO}}^{-}\left(\mathrm{q}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\rightleftharpoons \mathrm{HXO}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)$

is $0.3\times {10}^{-6}$ then find the value of dissociation constant (K_a) for HXO?

1. $0.36\times {10}^{-8}$

2. $2.8\times {10}^{-8}$

3. $2.8\times {10}^{-10}$

4. $0.36\times {10}^{-6}$

The equilibrium constant value for the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right) \mathrm{is} 1.48\times {10}^{-5}$, the value for the reaction $1/2{\mathrm{N}}_2\left(\mathrm{g}\right)+3/2{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right) \mathrm{is} \mathrm{n}\times {10}^{-3}$ 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. $\frac{1}{2}\left[{\mathrm{N}}_2{\mathrm{O}}_5\right]+\left[{\mathrm{O}}_2\right]=\frac{1}{2}\left[\mathrm{NO}\right]$

${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

The equilibrium pressure at $25°\mathrm{C}$ is 0.660 atm. What is K_p for the reaction?

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 is

1. 0.444

2. 0.555

3. 0.333

4. 0.666

K_c for the reaction ${\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)+\mathrm{NO}\left(\mathrm{g}\right)$ is 16 at a given temperature. If we take one mole each of all the four gases in one litre vessel, the equilibrium concentration of SO₂ and SO₃ respectively in mol L^-1 are 

1. 0.4, 0.8

2. 0.8, 0.16

3. 1.6, 0.8

4. 0.4, 1.6

The ratio of \({{K_{P}}\over{K_{C}}}\) for the reaction

$\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)$ $\mathrm{is:}$