Vapour density of ${\mathrm{N}}_2{\mathrm{O}}_4$ when heated to $100°\mathrm{C}$ becomes 24.5. its degree of dissociation at this temperature is

1. 80%

2. 87.75%

3. 40.34%

4. 60%

For the equilibrium  SO₂CI₂(g) ⇌ SO₂(g) + CI₂(g)  volume is increased.
When the equilibrium is re-established then: 

1. amount of  SO₂(g)  will decrease

2. amount of  SO₂CI₂(g)  will increase

3. amount of CI₂(g)  will increase

4. amount of CI₂(g) will remain unchanged

In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:

$\mathrm{Consider\; the\; given\; reaction:\; 2}\mathrm{HI}\stackrel{}{\rightleftharpoons }{\mathrm{H}}_2+{\mathrm{I}}_2$ 
At 22% dissociation of HI, what would be the value of equilibrium constant?

1. 0.04

2. 0.0198

3. 0.5

4. 1.2527

The degree of hydrolysis of the salt is independent of the concentration of a solution: 
1. NH₄CI
2. NH₄CN
3. (NH₄)₂SO₄
4. All of the above

The dissociation of solid ${\mathrm{NH}}_4\mathrm{SH}$ in a closed container produces a pressure of 4 atm at $95°\mathrm{C}$, then ${\mathrm{K}}_{\mathrm{p}}$ for the reaction will be:

${\mathrm{NH}}_4\mathrm{SH}\left(\mathrm{s}\right)\stackrel{}{\rightleftharpoons }{\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

The number of ${\mathrm{H}}^{\oplus }$ ions present in 1 ml of a solution whose pH= 4 , is given as:

($N_A=$ $Avogadro\text{'}s$ $number$)

1. ${10}^{-7}{N}_A$

2. ${10}^{-8}{N}_A$

3. ${10}^{-16}{N}_A$

4. ${10}^{-14}{N}_A$

If the pH of an acidic buffer is 5.7 and ${\mathrm{pK}}_{\mathrm{a}}$ is 5 then the ratio of $\frac{\left[\mathrm{Salt}\right]}{\left[\mathrm{Acid}\right]}$ will be:

The addition of NH₄Cl to an NH₄OH solution introduces a common ion into the system. As a result, the pH of the solution:

Consider the following two reactions : 

$\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right);$ ${\mathrm{K}}_1=$ $4\times {10}^{-3}$

$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right);$ ${\mathrm{K}}_2=?$

If ${\mathrm{K}}_1$ $\mathrm{and}$ ${\mathrm{K}}_2$ are equilibrium constants, the value of ${\mathrm{K}}_2$ will be: