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

A weak base BOH with $K_{b }={10}^{-5}$ is titrated with a strong acid HCl. At $\frac{3}{4}th$ of the equivalence point pH of solution is

(1) 5+log3

(2) 5-log3

(3) 9.425

(4) 8.523

A 0.1 molar solution of weak base BOH is 1% dissociated. If 0.2 moles of BCl is added in 1 litre solution of BOH, the degree of dissociation of BOH will become

(1) $2\times {10}^{-3}$

(2) $5\times {10}^{-5}$

(3) 0.05

(4) 0.02

Assuming no change in volume, calculate the minimum mass of NaCl (approx.) necessary to dissolve 0.01 mol AgCl in 100 L solution.

[Given $K_{sp}\left(AgCl\right)={10}^{-10}; K_f\left(AgC{l}_2^{-}\right)=3\times {10}^5]$

1. 15 kg

2. 21 kg

3 10 kg

4 .17 kg

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

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

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

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

(1) NH₃         

(2) H₂O         

(3) B₂H₆           

(4) CH₄

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)