Chemical Kineti...

A reaction involving A, B and C as reactants is found to obey the rate law, rate = k [A]^x [B]^y [C]^z . When the concentrations of A, B and C are doubled separately, the rate is also found to increase two, zero and four times respectively. The overall order of the reaction is

For the reaction system,
2NO(g ) +O₂(g)→ 2NO ₂(g)
volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to O₂ and second order with respect to NO; the rate of reaction will

The rate equation for the reaction 2A + B → C is found to be rate = k [A] [B] The correct statement in relation to this reaction is that the

Which one of the following is wrongly matched ?

The decomposition of N₂ O₅ occurs as 2N₂ O₅ → 4NO₂ + O₂, and follows 1st order kinetics, hence

In the reaction, 2N₂O₅ → 4NO₂ + O₂, initial pressure is 500 atm and rate constant k is 3.38 × 10^-5 s ^-1. After 10 min the final pressure of N₂O₅ is

Mathematical expression for t_1/4 i.e. when (1/4)^th reaction is over following first order kinetics can be given by

A plot of 1/ T versus k for a reaction gives the slope -1 × 10⁴ K. The energy of activation for the reaction is (Given, R = 8.314 K^-1 mol^-1 )

The rate of reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R = 8.314 JK^-1 mo1^-1 and log 2 = 0.301)