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

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

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

Determine the value of equilibrium constant (K_c) for the reaction

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

If 10 moles of A₂; 15 moles of B₂ and 5 moles of AB are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of AB is 7.5 M:

1. 4.5

2. 1.5

3. 0.6

4. None of the above

A 1 M solution of glucose reaches dissociation equilibrium given below.

${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\rightleftharpoons 6\mathrm{HCHO}$

If the equilibrium constant is $0.167x{10}^{-22}$, the concentration of HCHO in the equilibrium is

1. $1.60\times {10}^{-8<mspace\; width="1em"></mspace>}\mathrm{M}$

2. $3.20\times {10}^{-6}<mspace\; width="1em"></mspace>\mathrm{M}$

3. $3.20\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}$

4. $1.60\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}$

For the dissociation reaction ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$ the degree of dissociation $\left(\mathrm{\alpha }\right)$ in terms of K_p and total equilibrium pressure P is:

1. $\mathrm{\alpha }=\sqrt{\frac{4\mathrm{P}+{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{p}}}}$

2. $\mathrm{\alpha }=\sqrt{\frac{{\mathrm{K}}_{\mathrm{p}}}{4\mathrm{P}+{\mathrm{K}}_{\mathrm{p}}}}$

3. $\mathrm{\alpha }=\sqrt{\frac{{\mathrm{K}}_{\mathrm{p}}}{4\mathrm{P}}}$

4. None of these

When CO₂ dissolves in water, the following equilibrium is established.

${\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{H}}_3{\mathrm{O}}^{+}+\mathrm{H}{{\mathrm{CO}}_3}^{-}$

The equilibrium constant is $3.8\times {10}^{-7}$ and at pH=6.0, the ratio $\frac{\left[{{\mathrm{HCO}}_3}^{-}\right]}{\left[{\mathrm{CO}}_2\right]}$ will be

1. $3.8\times {10}^{-13}$

2. $3.8\times {10}^{-1}$

3. 6.0

4. 13.4

At certain temperature compound AB₂(g) dissociates according to the reaction

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

The value of K_p in terms of degree of dissociation $\text{'}\mathrm{\alpha }\text{'}$ and total pressure 'P' is

1. $\mathrm{P}\frac{{\mathrm{\alpha }}^3}{2}$

2. $\mathrm{P}\frac{{\mathrm{\alpha }}^2}{3}$

3. $\mathrm{P}\frac{{\mathrm{\alpha }}^3}{3}$

4. $\mathrm{P}\frac{{\mathrm{\alpha }}^2}{2}$

When NaNO3​ is heated in a closed vessel, O2​ is liberated and NaNO2​ is left behind. At equilibrium:

1. Addition of NaNO2​ favours reverse reaction

2. Addition of NaNO3​ favours forward reaction

3. Increasing temperature favours forward reaction.

4. None of these