For the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>500°\mathrm{C},$ 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, K_c for the following reaction is \(10^4 \rm { ~mol^{-1} ~L}\).
\(X(g) + Y(g) \rightleftharpoons Z(g)\)
At equilibrium, it was observed that,
\(\rm{[X] = \dfrac{1}{2}[Y] = \dfrac{1}{2} [Z]}\)

What is the value of [Z] at equilibrium?

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%

K_p has the value of 10^-6 atm³ and 10^-4 atm³ at 298 K and 323 K respectively for the reaction:
\(\mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{~s}) \rightleftharpoons \mathrm{CuSO}_4(\mathrm{~s})+3 \mathrm{H}_2 \mathrm{O}(\mathrm{~g})\)
\(\Delta_{\mathrm{r}} \mathrm{H}^{\circ} \text { for the reaction is: }\)

Assume that the decomposition of HNO₃ can be represented by the following equation

$4{\mathrm{HNO}}_3\left(\mathrm{g}\right)\rightleftharpoons 4{\mathrm{NO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$

and the reaction approaches equilibrium at 400K temperature and 30 atm pressure. At equilibrium, partial pressure of HNO₃ is 2 atm. Calculate K_c in (mol/L)³ at 400 K:

(Use : R=0.08 atm-L/mol-K)

1. 4

2. 8

3. 16

4. 32