$\frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$ for the gaseous reaction:

$$\begin{gathered} \mathrm{I}. 2\mathrm{A} + 3\mathrm{B} \rightleftharpoons 2\mathrm{C} \\ \mathrm{II}. 2\mathrm{A}\rightleftharpoons 4\mathrm{B} \\ \mathrm{III}. \mathrm{A}+\mathrm{B}+2\mathrm{C} \rightleftharpoons 4\mathrm{D} \end{gathered}$$

Would be respectively:

(1) (RT)^-3, (RT)², (RT)⁰ 

(2) (RT)^-3, (RT)-², (RT)^-1 

(3) (RT)^-3, (RT)², (RT) 

(4) None of the above

How many grams of CaC₂O₄ (molecular weight =128) on dissolving in distilled water will give a saturated solution

[K_sp (CaC₂O₄) = 2.5x10^-9 mol²l^-2

1. 0.0064 g             2. 0.1280 g

3. 0.0128 g             4. 1.2800 g

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