An element X being with oxygen and CO present in air as

$\mathrm{X}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{XO}}_2\left(\mathrm{g}\right); {\mathrm{K}}_{{\mathrm{p}}_1}=27$
$\mathrm{X}\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{XCO}\left(\mathrm{g}\right); {\mathrm{K}}_{{\mathrm{p}}_2}={10}^4$

When X at 1 atm is treated with air, 25% of it is bound to CO(g). The partial pressure of CO(g) in air at equilibrium, if partial pressure of O₂(g) in air at equilibrium is 0.2 atm, would be

1. $1.9\times {10}^4 \mathrm{atm}$

2. $1.9\times {10}^{-4} \mathrm{atm}$

3. $2.08\times {10}^4 \mathrm{atm}$

4. $2.08\times {10}^{-4} \mathrm{atm}$

For the reaction (i) and (ii)

$\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right) ...........\left(\mathrm{i}\right)$
$\mathrm{X}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{Y}\left(\mathrm{g}\right) .............\left(\mathrm{ii}\right)$

Given, ${\mathrm{K}}_{{\mathrm{p}}_1}:{\mathrm{K}}_{{\mathrm{p}}_2}=9:1.$ If degree of dissociation of A(g) and X(g) are same then the ratio of total pressure in equilibrium (i) and (ii) will be

1. 36:1

2. 0.5:1

3. 1:1

4. 3:1

For the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right) \mathrm{at} 500°\mathrm{C},$ the value of K_p is $1.44\times {10}^{-5}$ when the partial pressure are measured in atmosphere. The value of K_c with concentration in mol L^-1 is

1. $\frac{1.44\times {10}^{-5}}{{(8.314\times 773)}^{-2}}$

2. $\frac{1.44\times {10}^{-5}}{{(0.082\times 500)}^{-2}}$

3. $\frac{1.44\times {10}^{-5}}{{(0.081\times 773)}^{-2}}$

4. $\frac{1.44\times {10}^{-5}}{{(0.082\times 773)}^{-2}}$

The degree of dissociation of PCl₅ at one atmosphere is 0.3. The pressure at which PCl₅ is dissociated to 50% is

1. 0.273 atm

2. 0.3 atm

3. 1.34 atm

4. 2.73 atm

At 550 K, the K_c for the following reaction is ${10}^4 {\mathrm{mol}}^{-1} \mathrm{L}.$

$\mathrm{X}\left(\mathrm{g}\right)+\mathrm{Y}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{Z}\left(\mathrm{g}\right)$

At equilibrium, it was observed that

$\left[\mathrm{X}\right]=\frac{1}{2}\left[\mathrm{Y}\right]=\frac{1}{2}\left[\mathrm{Z}\right]$

What is the value of [Z] at equilibrium?

1. ${10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1}$

2. $2\times {10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1}$

3. $2\times {10}^4 \mathrm{mol} {\mathrm{L}}^{-1}$

4. ${10}^4 \mathrm{mol} {\mathrm{L}}^{-1}$

An exothermic reaction is represented by the graph:

1

2.

3. 

4. 

For the reversible system ${\mathrm{PCl}}_3+{\mathrm{Cl}}_2\rightleftharpoons {\mathrm{PCl}}_5,$ the relationship between degree of dissociation $\left(\mathrm{\alpha }\right)$ of PCl₅ and the equilibrium constant K_p of the above equilibrium is

1. $\frac{{\mathrm{K}}_{\mathrm{p}}}{\sqrt{\mathrm{P}+{\mathrm{K}}_{\mathrm{p}}}}$

2. $\sqrt{\frac{{\mathrm{K}}_{\mathrm{p}}}{1+\mathrm{P}.{\mathrm{K}}_{\mathrm{p}}}}$

3. $\frac{1}{\sqrt{\mathrm{P}+{\mathrm{K}}_{\mathrm{p}}}}$

4. $\sqrt{\frac{1}{1+\mathrm{P}.{\mathrm{K}}_{\mathrm{p}}}}$

One mole of N₂O₄(g) at 300 K is kept in a closed container under one atmospheric pressure. It is heated to 600 K when 20% by mass of N₂O₄(g) decomposes to NO₂(g).
The resultant pressure will be:

1. 1.0 atm

2. 2.4 atm

3. 2.0 atm

4. 1.2 atm

The equilibrium constant (K) of the reaction, $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$ at 298 K is 100. If the rate constant of the forward reaction is $4\times {10}^5$, the rate constant of the reverse reaction is

1. 4

2. $4\times {10}^2$

3. $4\times {10}^3$

4. $4\times {10}^5$

One mole of N₂O₄(g) at 310 K is 25% dissociated at 1 atm pressure. The percentage dissociation at 0.1 atm and 310 K is

1. 25%

2. 50%

3. 76%

4. 63%