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

If $\mathrm{pKa}=-\log {\mathrm{K}}_{\mathrm{a}}=4 \mathrm{and} {\mathrm{K}}_{\mathrm{a}}={\mathrm{Cx}}^2$ then Van't Hoff factor of weak monobasic acid when C=0.01 M is

1. 1.02

2. 1.01

3. 1.20

4. 1.10

The equilibrium constant (K_p) for the decomposition of water

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to {\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$

is given by

1. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{1}{2}}}}{\sqrt{2}}$

2. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{3}{2}}}}{(1-\mathrm{\alpha }){(2+\mathrm{\alpha })}^{{\displaystyle \frac{1}{2}}}}$

3. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{1}{2}}}}{(1+\mathrm{\alpha }){(2-\mathrm{\alpha })}^{{\displaystyle \frac{1}{2}}}}$

4. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^{3/2}{\mathrm{P}}^{1/2}}{(1-\mathrm{\alpha }){(2+\mathrm{\alpha })}^{1/2}}$

Where $\mathrm{\alpha }$ is the degree of dissociation and p is the pressure of the reaction mixture at equilibrium.

Which of these can not be a Bronsted acid?

1. ${\mathrm{HCO}}_3^{-}$

2. ${\mathrm{HCOO}}^{-}$

3. ${\mathrm{H}}_2{\mathrm{PO}}_3^{-}$

4. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

In ${\mathrm{HS}}^{-}, {\mathrm{I}}^{-}, {\mathrm{RNH}}_2 \mathrm{and} {\mathrm{NH}}_3$ order of proton accepting tendency will be

1. ${\mathrm{I}}^{-}>{\mathrm{NH}}_3>{\mathrm{RNH}}_2>{\mathrm{HS}}^{-}$

2. ${\mathrm{HS}}^{-}>{\mathrm{RNH}}_2>{\mathrm{NH}}_3>{\mathrm{I}}^{-}$

3. ${\mathrm{RNH}}_2>{\mathrm{NH}}_3>{\mathrm{HS}}^{-}>{\mathrm{I}}^{-}$

4. ${\mathrm{NH}}_3>{\mathrm{RNH}}_2>{\mathrm{HS}}^{-}>{\mathrm{I}}^{-}$

Which one of the following orders of acid strength is correct?

1. $\mathrm{RCOOH}>\mathrm{HC}\equiv \mathrm{CH}>\mathrm{HOH}>\mathrm{ROH}$

2. $\mathrm{RCOOH}>\mathrm{ROH}>\mathrm{HOH}>\mathrm{HC}\equiv \mathrm{CH}$

3. $\mathrm{RCOOH}>\mathrm{HOH}>\mathrm{ROH}>\mathrm{HC}\equiv \mathrm{CH}$

4. $\mathrm{RCOOH}>\mathrm{HOH}>\mathrm{HC}\equiv \mathrm{CH}>\mathrm{ROH}$

A centinormal solution of a monobasic acid is 100% ionized. Its pH is

1. 2

2. 4

3. 3

4. 1

The mixture that can act like a buffer is:

1. ${\mathrm{CH}}_3\mathrm{COOH} + {\mathrm{CH}}_3\mathrm{COONa}$

2. ${\mathrm{NH}}_4{\mathrm{NO}}_3+{\mathrm{NH}}_4\mathrm{OH}$

3. $50 \mathrm{ml} 0.1 \mathrm{m} \mathrm{NaCN}+30 \mathrm{ml} 0.1 \mathrm{m} \mathrm{HCl}$

4. All of the above