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

${\mathrm{CuSO}}_4.3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{CuSO}}_4\left(\mathrm{s}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$
${∆}_{\mathrm{r}}\mathrm{H}° \mathrm{for} \mathrm{the} \mathrm{reaction} \mathrm{is}:$

1. 7.7 kJ/mol

2. -147.41 kJ/mol

3. 147.41 kJ/mol

4. None of these

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

A 250 ml flask containing NO(g) at 0.46 atm is connected to a 100 ml flask containing oxygen gas at 0.86 atm by means of a stop cock at 350 K, the gases are mixed by opening the stop cock where the following equilibrium is established.

$\underset{\mathrm{g}}{2\mathrm{NO}}+{\mathrm{O}}_2\to \underset{\mathrm{g}}{2{\mathrm{NO}}_2}\rightleftharpoons \underset{\mathrm{g}}{{\mathrm{N}}_2{\mathrm{O}}_4}$

The first reaction is complete while the second is at equilibrium. If thetotal pressure is 0.37 atm, K_p is

1. 0.645 atm^-1 

2. 1.290 atm^-1 

3. 20 atm^-1 

4. 5.46 atm^-1 

The equilibrium constant for the reactions

${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3 \mathrm{and} \frac{1}{2}{\mathrm{N}}_2+\frac{3}{2}{\mathrm{H}}_2\rightleftharpoons {\mathrm{NH}}_3$

are K₁ and K₂ respectively. The correct relationship between K₁ and K₂ is

1. ${\mathrm{K}}_1=\frac{{\mathrm{K}}_2}{2}$

2. ${\mathrm{K}}_2=\sqrt{{\mathrm{K}}_1}$

3. ${\mathrm{K}}_2={{\mathrm{K}}_1}^2$

4. ${\mathrm{K}}_1={\mathrm{K}}_2$

One mole of N₂(g) is mixed with 2 moles of H₂(g) in a 4 litre vessel. 50% of N₂(g) is converted to NH₃(g) by the following reaction:

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

What will be the value of K_c for the following equilibrium?

${\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{3}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)$

1. 256

2. 16

3. $\frac{1}{16}$

4. None of the above