Following data are obtained for the reaction :
N₂O₅ → 2NO₂ + ½O₂

(a) Show that it follows first order reaction.
(b) Calculate the half-life.
(Given log 2 = 0.3010 log 4 = 0.6021)

For the reaction,$2N_2{O}_5 \left(g\right) \stackrel{ }{\to } 4 N{O}_2 \left(g\right) + O_2 \left(g\right)$ the rate of formation of NO₂ (g)  is 2.8 x 10^-3 Ms^-1. Calculate the rate of disappearance of N₂O₅ (g).

A first-order reaction is 50% completed in 40 minutes at 300 K and in 20 minutes at 320 K. Calculate the activation energy of the reaction.

(Given: log 2 = 0.3010, log 4 = 0.6021, R = 8.314 JK^–1 mol^–1)

Rate law for the reaction, A+ B → product is rate = k[A]²[B] What is the rate constant; if rate of reaction at a given temperature is 0.22 Ms^-1, when [A]= 1 M band [BJ= 0.25 M?

• 3.52 M^-2s^-1

• 0.88  M^-2s^-1

• 1.136  M^-2s^-1

• 0.05  M^-2s^-1

305.

Decomposition of H₂O₂ follows a first order reaction. In fifty minutes the concentration of H₂O₂ decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H₂O₂ reaches 0.05 M, the rate of formation of O₂ will be:

• 6.93×10⁻⁴ mol min⁻¹

• 2.66 L min⁻¹ at STP

• 1.34×10⁻² mol min⁻¹

• 1.34×10⁻² mol min⁻¹

Higher order (>3) reactions are rare due to:

• the increase in entropy and activation energy as more molecules are involved.

• shifting of equilibrium towards reactants due to elastic collisions

• loss of active species on a collision

• loss of active species on a collision

The resistance of 0.2 M solution of an electrolyte is 50 Ω. The specific conductance of the solution of 0.5 M solution of the same electrolyte is 1.4 S m^-1 and resistance of the same solution of the same electrolyte is 280 Ω. The molar conductivity of 0.5 M solution of the electrolyte in Sm^-2 mol^-1 is

• 5 x 10^-4

• 5 x 10^-3

• 5 x 10³

• 5 x 10³

For the non- stoichiometric reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiment, all at 298 K.

The rate of a reaction doubles when its temperature changes from 300K to 310K. Activation energy of such a reaction will be (R = 8.314 JK^–1 mol–1 and log 2 = 0.301)

• 53.6 kJ mol^-1

• 48.6 kJ mol^-1

• 58.5 kJ mol^-1

• 58.5 kJ mol^-1

For a first order reaction, (A) → products, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is

• 1.73 x 10^–5 M/ min

• 3.47 x 10^–4 M/min

• 3.47 x 10^–5 M/min

• 3.47 x 10^–5 M/min