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

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. $\frac{\mathrm{P}}{4}$