What will be the change in the concentration of Cl₂ when the equilibrium concentration of PCl₃ is doubled in the reaction:

PCl₅(s) ⇌ PCl₃(g) + Cl₂(g)?

1. Cl₂ becomes half of its initial concentration

2. Cl₂ becomes one-fourth of its initial concentration

3. Cl₂ becomes four times its initial concentration

4. Cl₂ becomes twice its initial concentration

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

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