Ostwald dilution law for weak electrolyte HA can be given as

$\left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0$
$\left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above}$

If carbon dioxide is 2% dissociated at equilibrium 2CO₂ (g)$\rightleftharpoons$2CO(g) + O₂(g). The mole fraction of CO₂ at equuilibrium is

(1) 1.01/0.98            (2) 0.98/1.01

(3) 0.01/0.98            (4) 0.098/1.01

Which of the following is least likely to behave as Lewis base?
(1) NH₃

(2) BF₃

(3) OH^-

(4) H₂O

In which of the following equilibrium K_c and K_p are not equal?

(1) 2NO(g) $\rightleftharpoons$N₂(g) + O₂(g)

(2) SO₂(g) + NO₂(g) $\rightleftharpoons$SO₃(g) + NO(g)

(3) H₂(g) + I₂(g) $\rightleftharpoons$2HI(g)

(4) 2C(s) + O₂(g) $\rightleftharpoons$2CO₂(g)

Which one of the following molecular hydrides acts as a Lewis acid?

(1) NH₃         

(2) H₂O         

(3) B₂H₆           

(4) CH₄

If the concentration of OH^- ions in the reaction

Fe(OH)3 (s) $\rightleftharpoons$Fe³⁺ (aq) + 3OH^-(aq) is decreased to 1/4 times, then equilibrium concentration of Fe³⁺ will increase by

(a) 8 times                            (b) 16 times

(c) 64 times                          (d) 4 times

Calculate the pOH of a solution at 25$°$C that contains 1x10^-10 M of hydronium ions.

(a) 7.00                                 (b) 4.00

(c) 9.00                                 (d) 1.00

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)

(1) 1.2

(2) 2.25

(3) 2.1

(4) 3.6

For the equilibrium:

$LiCl·3N{H}_3\rightleftharpoons LiCl·N{H}_3+2N{H}_3·K_P=9 at{m}^2$

At $27°C,$ a 8.2L vessel contains 0.1 mol of LiCl.$N{H}_3\left(s\right)$. How many moles of $N{H}_3$ should be added to the flask at this temperature of derive the backward reaction for completion?

(1) 20.5 mol

(2) 3 mol

(3) 1.2 mol

(4) 0.21 mol

Ammonia at a pressure 10 atm and $C{O}_2$ at a pressure at 20 atm are introduced into an evacuated chamber. If $K_p$ for the reaction

$N{H}_{2}COON{H}_4\left(s\right) \rightleftharpoons 2N{H}_3\left(g\right)+C{O}_2\left(g\right)$ is 2020 $at{m}^2$ at 400K then the final pressure in the chamber would be

(1) Less than 30 atm

(2) More than 30 atm

(3) Equal to 30 atm

(4) Unpredictable