For the reaction, 2NO(g) + Cl₂(g) $\rightleftharpoons$2NOCl(g). which relation is true ?

• K_P=K_c × RT

• ${\mathrm{K}}_{\mathrm{P}}= \frac{{\mathrm{K}}_{\mathrm{c}}}{\mathrm{RT}}$

• ${\mathrm{K}}_{\mathrm{P}}= {\mathrm{K}}_{\mathrm{c}}(\mathrm{RT}{)}^2$

• ${\mathrm{K}}_{\mathrm{P}}= \frac{{\mathrm{K}}_{\mathrm{c}}}{{\left(\mathrm{RT}\right)}^2}$

If the molar solubility of X₃B₃(AlF₆)₂ at 298 K is x, the solubility product K_sp is

• 18x³

• 27x⁴

• 27x⁸

• 2916x⁸

The pH of 0.05 M solution of a strong dibasic acid is

• 0.0

• 1.0

• 0.2

• 0.5

274.

For the equilibrium reaction,

2SO₂ (g) + O₂ (g) $\rightleftharpoons$ 2SO₃ (g) + $∆$H

the increase in temperature

• favours the formation of SO₃

• favours the decomposition of SO₃

• does not affect the equilibrium

• stops the reaction

5 millimoles of caustic potash and 5 millimoles of oxalic acid are mixed and dissolved in 100 mL water. The solution will be

• basic

• acidic

• neutral

• cannot say

Which solution is a buffer?

• Acetic acid + NaOH (equimolar ratio)

• Acetic acid + NaOH (1 : 2 molar ratio)

• Acetic acid + NaOH (2 : 1 molar ratio)

• HCl + NaOH (equimolar ratio)

The solubility of Al(OH)₃ is 'S' mol L^-1. The solubility product will be

• S²

• S³

• 27 S⁴

• 27 S³

If in the reaction N₂O₄ $\rightleftharpoons$2NO₂: $\mathrm{\alpha }$ is the degree of dissociation of N₂O₄ then total number of moles at equilibrium is

• (1-α)

• (1+α)

• (1-α)²

• (1+α)²

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

CO (g) + $\frac{1}{2}$ O₂ (g) $\rightleftharpoons$ CO₂ (g) is

• RT

• $\frac{1}{\sqrt{\mathrm{RT}}}$

• $\sqrt{\mathrm{RT}}$

• $\frac{1}{\mathrm{RT}}$

In the equilibrium mixture, KI+ I₂ $\rightleftharpoons$KI₃ the concentration of KI and I₂ and three fold respectively . The concentration of KI₃ becomes

• two fold

• three fold

• five fold

• six fold