The addition of a small amount of argon at a constant volume will not affect the equilibrium of the following reaction:

1.	H2(g)+I2(g)⇌2HI(g)
2.	PCl5(g)⇌ PCl3(g)+Cl2(g)
3.	N2(g)+3H2(g)⇌2NH3(g)
4.	The equilibrium will remain unaffected in all the three cases.

The correct decreasing order of basic strength of the following species is.

${\mathrm{H}}_2\mathrm{O},{\mathrm{NH}}_3,{\mathrm{OH}}^{-},{\mathrm{NH}}_2^{}$

$1.<mspace\; width="1em"></mspace>{\mathrm{NH}}_2^{-}>{\mathrm{OH}}^{-}>{\mathrm{NH}}_3>{\mathrm{H}}_2\mathrm{O}$
$2.<mspace\; width="1em"></mspace>{\mathrm{OH}}^{-}>{\mathrm{NH}}_2^{-}>{\mathrm{H}}_2\mathrm{O}>{\mathrm{NH}}_3$
$3.<mspace\; width="1em"></mspace>{\mathrm{NH}}_3>{\mathrm{H}}_2\mathrm{O}>{\mathrm{NH}}_2^{-}>{\mathrm{OH}}^{-}$
$4.<mspace\; width="1em"></mspace>{\mathrm{H}}_2\mathrm{O}>{\mathrm{NH}}_3>{\mathrm{OH}}^{-}>{\mathrm{NH}}_2^{-}$

At 500 K, equilibrium constant, K_c, for the following reaction is 5.

$\frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right)\rightleftharpoons \mathrm{HI}\left(\mathrm{g}\right)$

What would be the equilibrium constant K_c for the reaction?

$2\mathrm{HI}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$

1.  0.04

2.  0.4

3.  25

4.  2.5

On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,

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

Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?

Which of the following alternatives best describes the reaction A ⇌ B at its halfway point?
1. \(\Delta G^{\ominus}=0\)
2. \(\Delta G^{\ominus}>0\)
3. \(\Delta G^{\ominus}<0\)
4. \(\Delta G^{\ominus}=-RTlnK\)

${\mathrm{}}_{}$
Find the pH of ammonium acetate solution when the value of Ka for CH₃COOH is 1.8 × 10⁻⁵
and Kb for NH₄OH is 1.8 × 10⁻⁵.

1. 7.005

2. 4.75

3. 7.0

4. Between 6 and 7

The value of the pH of \(0.01 \) \(\text{mol dm}^{-3}   \)\(\text{CH}_3\text{COOH}\) \(\left(K_a=1.74 \times 10^{-5}\right)\)  is:

The mixture that will produce a buffer solution when mixed in equal volumes is:

Acidity of BF₃ can be explained on the basis of: 

1. Arrhenius concept

2. Bronsted Lowry concept 

3. Lewis concept

4. Bronsted Lowry as well as Lewis concept