Calculate the activation energy - find out the rate

Question

Q.1. Find out the order of the following reaction. Also evaluate the unit of rate constant of the recation 'k.CH₃CHO → CH₄ +CO

rate = - d[CH₃CHO]/dt = k[CH₃CHO]^3/2

Q.2 Rate of formation of NH₃ is 3.0 x 10^-4 molL^-1sec^-1. Find the rate of consumption of N₂ & H₂.

Q.3 Prove that the time required to complete 99.9% reaction is the 10 times of the half-life of a first order chemical kinetics.

Q.4 Establish the integrated rate expression of first order reaction.

Q.5 The experimental data of a chemical reaction 2A + B₂ → 2AB is given below

Run	[A] (mol L-1)	[B2] (mol L-1)	[rate] (mol L-1sec-1)
1	0.50	0.50	1.6??10-4
2	0.50	1.00	3.2??10-4
3	1.00	1.00	3.2??10-4

Write down the most probable rate equation for the reaction. Explain.

Q.6 Consider the following reaction 2 NO_2(g) → 2NO_(g) + O_2(g)
At 650k, the rate constant 1.66 sec^-1.

At 700k, the rate constant 7.39 sec^-1.

Calculate the activation energy.

Q.7 For a first order reaction log k vs 1/t plot has a slop of -6000 K. Calculate activation energy of the reaction.

Q.8 The integrated rate expression of a n-th order reaction is given below.

1/(n-1).[1/(C^n-1) - 1/(C₀^n-1)] = kt

Find out the rate expression of zero order reaction. Calculate the time of completion of reaction.