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

1. ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>∆\mathrm{H}=+\mathrm{ve}$

2. $2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>∆\mathrm{H}=-\mathrm{ve}$

3. $3{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>∆\mathrm{H}=-\mathrm{ve}$

4. ${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right);<mspace\; width="1em"></mspace>∆\mathrm{H}=+\mathrm{ve}$

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 $2\mathrm{B}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\mathrm{C}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>2\mathrm{A}$(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:

$$\begin{gathered} {\mathrm{H}}_3{\mathrm{PO}}_4\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_1, \\ <mspace\; width="1em"></mspace>{\mathrm{H}}_2{\mathrm{PO}}_4\rightleftharpoons {\mathrm{H}}^{+}+{{\mathrm{HPO}}_4}^{2-}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_2<mspace\; width="1em"></mspace>\mathrm{and} \\ <mspace\; width="1em"></mspace>{{\mathrm{HPO}}_4}^{2-}\rightleftharpoons {\mathrm{H}}^{+}+{{\mathrm{PO}}_4}^{3-}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_3. \end{gathered}$$

The equilibrium constant (K) for

${\mathrm{H}}_3{\mathrm{PO}}_4\rightleftharpoons 3{\mathrm{H}}^{+}+{{\mathrm{PO}}_4}^{3-}<mspace\; width="1em"></mspace>\mathrm{will}<mspace\; width="1em"></mspace>\mathrm{be}$

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,

${\mathrm{XeF}}_6\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeOF}}_4\left(\mathrm{g}\right)+2\mathrm{HF}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>........\left(\mathrm{i}\right)$

$\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{XeO}}_4\left(\mathrm{s}\right)+{\mathrm{XeF}}_6\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeOF}}_4\left(\mathrm{g}\right)+{\mathrm{XeO}}_3{\mathrm{F}}_2\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>......\left(\mathrm{ii}\right)$

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

${\mathrm{XeO}}_4\left(\mathrm{g}\right)+2\mathrm{HF}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XeO}}_3{\mathrm{F}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{is}$

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: \(CO + Cl_2 ⇌ COCl_2\)

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