For the reversible reaction,

N2(g)+3H2(g)⇌2NH3(g)

At 500°C, the value of K_p is 1.44×10^-5 when partial pressure is measured in atmospheres. The corresponding value of K_c, with concentration in mole L^-1, is

1. 1.44×10^-5(0.082×500)^-2

2. 1.44×10^-5/(8.314×773)^-2

3. 1.44×10^-5(0.082×773)^-2

4. 1.44×10^-5/(0.082×773)^-2

If N₂O₄ is dissociation to 33% and 40% at total pressure P₁ and P₂ atm respectively. The ratio of $\frac{{\mathrm{P}}_1}{{\mathrm{P}}_2}$ is

1. $\frac{8}{5}$

2. $\frac{5}{8}$

3. $\frac{9}{5}$

4. $\frac{5}{9}$

For which of the following reaction, ${\mathrm{K}}_{\mathrm{p}}={\mathrm{K}}_{\mathrm{c}}?$

1. $2\mathrm{NOCl}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

2. ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

3. ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HCl}\left(\mathrm{g}\right)$

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

In which of the following reactions, equilibrium is independent of pressure?

1. ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right); ∆\mathrm{H}=+\mathrm{ve}$

2. $2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right); ∆\mathrm{H}=-\mathrm{ve}$

3. $3{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right); ∆\mathrm{H}=-\mathrm{ve}$

4. ${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right); ∆\mathrm{H}=+\mathrm{ve}$

The equilibrium constant of mutarotation of $\mathrm{\alpha }$-D-glucose to $\mathrm{\beta }$-D-glucose is 1.8. What percent of the $\mathrm{\alpha }$-form remains under equilibrium?

1. 35.7

2. 64.3

3. 55.6

4. 44.4

For a gaseous equilibrium

$2\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right),$ K_p has a value of 1.8 at 700 C. What is the value of K_c for the equilibrium $2\mathrm{B}\left(\mathrm{g}\right) + \mathrm{C}\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{A}$(g)  at the same pressure?

1. 0.031

2. $1.3\times {10}^{-3}$

3. 44.4

4. 38

The equilibrium constants for the given reactions are:

$$\begin{gathered} {\mathrm{H}}_3{\mathrm{PO}}_4\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{H}}_2{{\mathrm{PO}}_4}^{-} \mathrm{is} {\mathrm{K}}_1, \\ {\mathrm{H}}_2{\mathrm{PO}}_4\rightleftharpoons {\mathrm{H}}^{+}+{{\mathrm{HPO}}_4}^{2-} \mathrm{is} {\mathrm{K}}_2 \mathrm{and} \\ {{\mathrm{HPO}}_4}^{2-}\rightleftharpoons {\mathrm{H}}^{+}+{{\mathrm{PO}}_4}^{3-} \mathrm{is} {\mathrm{K}}_3. \end{gathered}$$

The equilibrium constant (K) for

${\mathrm{H}}_3{\mathrm{PO}}_4\rightleftharpoons 3{\mathrm{H}}^{+}+{{\mathrm{PO}}_4}^{3-} \mathrm{will} \mathrm{be}$

1. ${\mathrm{K}}_1\times {\mathrm{K}}_2\times {\mathrm{K}}_3$

2. ${\mathrm{K}}_1/{\mathrm{K}}_2{\mathrm{K}}_3$

3. ${\mathrm{K}}_2/{\mathrm{K}}_1{\mathrm{K}}_3$

4. ${\mathrm{K}}_1+{\mathrm{K}}_2+{\mathrm{K}}_3$

The equilibrium constants for the reactions,

${\mathrm{XeF}}_6\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeOF}}_4\left(\mathrm{g}\right)+2\mathrm{HF}\left(\mathrm{g}\right) ........\left(\mathrm{i}\right)$

$\mathrm{and} {\mathrm{XeO}}_4\left(\mathrm{s}\right)+{\mathrm{XeF}}_6\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeOF}}_4\left(\mathrm{g}\right)+{\mathrm{XeO}}_3{\mathrm{F}}_2\left(\mathrm{g}\right) ......\left(\mathrm{ii}\right)$

are K₁ and K₂ respectively. The equilibrium constant (K) for the reaction

${\mathrm{XeO}}_4\left(\mathrm{g}\right)+2\mathrm{HF}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeO}}_3{\mathrm{F}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) \mathrm{is}$

1. ${\mathrm{K}}_1/{\mathrm{K}}_2$

2. ${\mathrm{K}}_2/{\mathrm{K}}_1$

3. K₁=2K₂

4. K₂=1K₁

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:

$\mathrm{CO}+{\mathrm{Cl}}_2\rightleftharpoons {\mathrm{COCl}}_2$

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