9.2 g N₂O₄ is heated in a 1L vessel till equilibrium state is established

N₂O₄ (g) $\rightleftharpoons$ 2NO₂ (g)

In equilibrium state 50% Np4 was dissociated, equilibrium constant will be (mol. wt. of N₂O₄ = 92)

• 0.1

• 0.4

• 0.3

• 0.2

Solubility product of PbCl₂ at 298 K is 1 x 10^-6. At this temperature solubility of PbCl₂ in mol/L is

• (1 x 10^-6)^1/2

• (1 x 10^-6)^1/3

• (0.25 x 10^-6)^1/3

• (2.5 x 10^-6)^1/2

Which of the following is the electron deficient molecule?

• B₂H₆

• C₂H₆

• PH₃

• SiH₄

Equilibrium constants K₁ and K₂ for the following equilibria
NO (g) + $\frac{1}{2}{\mathrm{O}}_2$ $\stackrel{{\mathrm{K}}_1}{\rightleftharpoons }$ NO₂(g) and

2NO₂(g) $\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }$ 2NO (g) + O₂(g)

are related as

• ${\mathrm{K}}_2 = \frac{1 }{{\mathrm{K}}_1}$

• ${\mathrm{K}}_2 = {\mathrm{K}}_1^2$

• ${\mathrm{K}}_2 = \frac{{\mathrm{K}}_1}{2}$

• ${\mathrm{K}}_2 =\frac{1}{{\mathrm{K}}_1^2}$

85.

H₂S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because: 

• presence of HCl decreases the sulphide ion concentration

• presence of HCl increases the sulphide ion concentration

• solubility product of group II sulphides is more than that of group IV sulphides

• sulphides of group IV cations are unstable in HCl

A + B $\rightleftharpoons$ C + D. If initially the concentration of A and B are both equal but at equilibrium, concentration of D will be twice of that of A, then what will be the equilibrium constant of reaction?

• 4/9

• 9/4

• 1/9

• 4

Given pH of a solutionA is 3 and it is mixed with another solution B having pH 2. If both mixed, then resultant pH of the solution will be :

• 3 : 2

• 1 : 9 

• 3 : 4

• 3 : 5

When NaNO₃ is heated in a closed vessel oxygen is liberated and NaNO₃ is left behind,

At equilibrium:

• addition of NaNO₂ favours reverse reaction

• addition of NaNO₃ favours reverse reaction

• increasing temperature favours forward reaction

• decreasing temperature favours backward reaction

${\mathrm{CaCO}}_{3 } \rightleftharpoons \mathrm{CaO} + {\mathrm{CO}}_2 \mathrm{reaction} \mathrm{in} \mathrm{lime} \mathrm{kiln} \mathrm{goes} \mathrm{to} \mathrm{completion} \mathrm{because}$:

• CaO does not react to CO₂  to give CaCO₃

• backward reaction is very low

• CO₂ formed escapes out

• None of the above

Consider the following reversible reaction at equilibrium:

${\text{2H}}_2\mathrm{O} \left(\mathrm{g}\right) \rightleftharpoons 2 {\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right) + {\mathrm{O}}_2 \left(\mathrm{g}\right) ; \mathrm{\Delta H} = +24.7 \mathrm{KJ}$

The maximum decomposition of H₂O(g) will occur by which of the following change in conditions.

• Increasing temperature and decreasing pressure

• Decrease temperature and increasing pressure

• Increasing both temperature and pressure

• Increasing temperature at constant pressure