The slope of the graph drawn between ln k and $\frac{1}{\mathrm{T}}$ as per Arrhenius equation gives the value (R = gas constant; E_a = Activation energy)

• $\frac{\mathrm{R}}{{\mathrm{E}}_{\mathrm{a}}}$

• $\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}}$

• $-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}}$

• $\frac{-\mathrm{R}}{{\mathrm{E}}_{\mathrm{a}}}$

$$\begin{gathered} \left(\mathrm{i}\right) {\mathrm{H}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+} \left(\mathrm{aq}\right) + {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(\mathrm{aq}\right) \\ \left(\mathrm{ii}\right) {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+} \left(\mathrm{aq}\right) + {\mathrm{HPO}}_4^{2-} \left(\mathrm{aq}\right) \\ \left(\mathrm{iii}\right) {\mathrm{HPO}}_4^{2-} \left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+}\left(\mathrm{aq}\right) + {\mathrm{PO}}_4^{3-}\left(\mathrm{aq}\right) \end{gathered}$$

The equilibrium constants for the above reactions at a certain temperature are K₁, K₂ and K₃ respectively. The equilibrium constant for the reaction ${\mathrm{H}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right) \rightleftharpoons 3{\mathrm{H}}^{+}\left(\mathrm{aq}\right) + {\mathrm{PO}}_4^{3-} \left(\mathrm{aq}\right)$ in terms of K₁, K₂ and K₃ is 

• K₁+ K₂ + K₂

• $\frac{{\mathrm{K}}_1}{{\mathrm{K}}_2+{\mathrm{K}}_3}$

• $\frac{{\mathrm{K}}_3}{{\mathrm{K}}_1{\mathrm{K}}_2}$

• K₁K₂K₃

The equilibrium constant (K_c) for the following equilibrium $2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$ at 563 K is 100. At equilibrium, the number of moles of SO₃ in the 10 litre flask is twice the number of moles of SO₂ , then the number of moles of oxygen is

• 0.4

• 0.3

• 0.2

• 0.1

The relation between K_p and K_c is correctly shown as

• K_c = K_p (RT)${}^{∆{\mathrm{n}}_{\mathrm{g}}}$

• K_p = K_c (RT)${}^{-∆{\mathrm{n}}_{\mathrm{g}}}$

• K_p = K_c (RT)${}^{∆{\mathrm{n}}_{\mathrm{g}}}$

• K_c = K_p (RT)${}^{-∆{\mathrm{n}}_{\mathrm{g}}}$

In the formation of SO₃ according to following equilibrium 2SO₂ + O₂ $\rightleftharpoons$ 2SO₃ + heat, which conditions favour the formation of SO₃?

• Low pressure

• Low concentration of oxygen

• Low temperature and use of catalyst

• High temperature without using catalyst

Which of the following mixtures forms an acid buffer?

• NaOH + HCl

• CH₃COOH + CH₃COONa

• NH₄OH + NH₄Cl

• H₂CO₃ + (NH₄)₂CO₃

When NH₄Cl is added to NH₄OH solution, the dissociation of ammonium hydroxide is reduced. It is due to

• common ion effect

• hydrolysis

• oxidation

• reduction

Strongest Bronsted base among the following anions is

• ClO^-

• ClO${}_2^{-}$

• ClO${}_3^{-}$

• ClO${}_4^{-}$

pH of a solution is 4. The hydroxide ion concentration of the solution would be

• 10^-4

• 10^-10

• 10^-2

• 10^-12

Heat of neutralisation of NH₄OH and HCl is

• equal to 13.7 kcal

• more than 13.7 kcal

• less than 13.7 kcal

• more than one is correct