If in the reaction N₂O₄ $\rightleftharpoons$ 2NO₂ , x is that part of N₂O₄ which dissociates, then the number of molecules at equilibrium will be :

• 1

• 3

• (1 + X)

• (1 + X)²

For the reaction, H₂ + I₂ $\rightleftharpoons$ 2HI, K = 47.6. If the initial number of moles of each reactant and product is 1 mole then at equilibrium

• [I₂] = [H₂] , [I₂] > [HI]

• [I₂] = [H₂] , [I₂] < [HI]

• [I₂] < [H₂] , [I₂] = [HI]

• [I₂] > [H₂] , [I₂] = [HI]

Calculate the overall complex dissociation equilibrium constant for the [Cu(NH₃)₄]²⁺ ions, given that stability  constant (${\mathrm{\beta }}_4$) for this complex is 2.1 $\times$ 10¹³.

• 8.27 $\times$ 10^-13

• 4.76 $\times$ 10^-14

• 2.39 $\times$ 10^-7

• 1.83 $\times$ 10¹⁴

The temperature dependence of a reaction is represented by the Arrhenius equation: 

ln k = -$\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{RT}}+\ln \mathrm{A}$

Which among the following is wrong conclusion about the given plot?

• Intercept of the line= ln A

• Slope = -$\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{RT}}$

• Reaction with high activation energy is more temperature sensitive than that of low activation energy (E_a).

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

Which of the following oxoacids of phosphorus is a reducing agent and a monobasic acid as well?

• H₄P₂O₅

• HPO₃

• H₃PO₃

• H₃PO₂

K_a for HCN is 5 x 10^-10 at 25°C. For maintaining a constant pH = 9, the volume of 5 M KCN solution required to be added to 10 mL of 2 M HCN solution is

• 4 mL

• 2.5 mL

• 2 mL

• 6.4 mL

Assertion : The second dissociation constant of fumaric acid is greater than maleic acid.

Reason : Higher the dissociation constant of acid, more is the acidic character.

• If both assertion and reason are true and reason is the correct explanation of assertion.

• If both assertion and reason are true but reason is not the correct explanation of assertion

• If assertion is true but reason is false.

• If both assertion and reason are false

NO₂ (brown colour gas) exists in equilibrium with N₂O₄ (colourless gas) as given by chemical equation.

$\underset{\left(\mathrm{brown}\right)}{2{\mathrm{NO}}_2} \rightleftharpoons \underset{\left(\mathrm{colourless}\right)}{{\mathrm{N}}_2{\mathrm{O}}_4}$

Mixture is slightly brown due to existence of NO₂. If pressure is increased :

• colour intensity is increased

• colour intensity is decreased

• colour intensity first increases and then decreases

• No change in colour intensity

K_P for the reaction A $\rightleftharpoons$ B is 4. If initially only A is present then what will be the partial pressure of B after equilibrium?

• 1.2

• 0.8

• 0.6

• 1

0.1 M solution of CH₃COOH should be diluted to how many times so that pH is doubled ?

• 4.0 times

• 5.55 x 10⁴ times

• 5.55 x 10⁶ times

• 10^-2 times