If K_p of the reaction $\mathrm{A}\left(\mathrm{g}\right)+2\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 3\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$ is 0.05 at 1000 K, then the value of K_c of the reaction

1. 20000 R

2. 0.02 R

3. $\frac{5\times {10}^{-5}}{\mathrm{R}}$

4. $5\times {10}^{-5}\mathrm{R}$

The reaction ${\mathrm{PCl}}_5\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$ is in equilibrium. If the equilibrium concentration of PCl₃(g) is doubled, then the concentration of Cl₂(g) would become

1. 1/2 of its initial value

2. 1/4 of its initial value

3. four times of its initial value

4. two times of its initial value

In the reaction, the equilibrium concentrations of PCl₅ and PCl₃ are 0.4 and 0.2 mole/liter respectively. If the value of K_c is 0.5, what is the concentration of Cl₂ in mole/liter?

1. 2.0

2. 1.5

3. 1.0

4. 0.5

4 moles each of SO₂ and O₂ gases are allowed to react to form SO₃ in a closed vessel. At equilibrium, 25% of O₂ is used up. The total number of moles of all the gases at equilibrium is

1. 6.5

2. 7.0

3. 8.0

4. 2.0

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