The decomposition of `NH_3` on platinum surface is zero order reaction. What are the rates of production of `N_2` and `H_2` if `k = 2.5xx10^-4 mol^-1 s^-1`?

The decomposition of NH_3 on plantinum surface is a zero order reaction. What are the rates of productions of N_2 and H_2 if K = 2.5xx10^(-4)mol^(-1)Ls^(-1) ?

Identify the reaction order from each of the following rate constants. k=1.4xx10^(-5)mol^(-1)Ls^(-1)

For a decomposition reaction, the values of rate constants at two different temperatures are given below: K_1 = 2.15xx10^-8 Lmol^-1s^-1 at 650k K_2 = 2.39xx10^-7 Lmol^-1s^-1 at 700k Calculate the value of activation energy for the reaction (R = 8.314 JK^-1 mol^-1 )

Identify the reaction order from each of the following rate constants. k=2.3xx10^(-4)s^(-1)

The rate constant of a reaction is 3xx10^2 min^-1 . What is the order of the reaction?

Find out half-life time of first order reaction with rate constant k=2.31xx10^(-14)s^(-1) .

Complete the following acid-base reactions and name the products: (C_2H_5)_3N + HCl rarr

Find out 2/3 life of a first order reaction in which K = 5.48xx10^-14s^-1