For the decomposition of azoisopropane to hexane and nitroger at `543 K`, the following data are obtained. Calculate the rate constant. t=0,360S,720S and P=35,54,63 respectively.

Rate of a reaction is the change in concentration of any one of the reactants or any one of the products in unit time. Calculate the time required for the completion of 90% of a first order reaction( k=0.2303s^(-1) )

The temperature dependence of the rate of a chemical reaction can be accurately explained by Arrhenius equation. With the help of Arrhenius equation, calculate the rate constant for the first order reaction C_2H_5I(g)toC_2H_(4(g))+HI_((G))at700K .Energy of activation (Ea)for the reaction is 209kjmol_(-1) and rate constant at 600K is 1.60xx10^(-5)s^(-1) [Universal gas constant R= 8.314JK^(-1)mol^(-1)]

From the following data show that the decomposition of hydrogen peroxide in aqueous solution is a first order reaction what is the value of the rate constant Time (t) in minutes 0 10 20 30 40 V(mL) 25.0 20.0 15.7 12.5 9.6 Where V is volume of kMnO_(4) solution required decompose a definite volume of hydrogen peroixde

The catalytic decomposition of H_(2)O_(2) was studied by titrating it at different intervals with KMnO_(4) solution.Calcualte the rate constant from the following data assuming the reaction to be of the first order time t(seconds): 0 600 1200 KMnO_(4) (mL) :22.8 13.8 8.2

The Experiment data for decomposition of N{2}O{5} [2N{2}O{5}rarr4NO{5}+O{2}] is gas phase at 318 K are given below: i) Plot [N{2}O{5}] against t. ii) Find the half-life period for the reaction. iii) Draw a graph between log [N{2}){5}] and t iv) What is the rate law Calculate the rate constant. vi) Calculate the half life period from K and compare it with(2) t/s=0,400,800,1200,1600,2000,2400,2800,3200 and [N2O5]=1.63,1.36,1.14,0.93,0.78,0.64,0.53,0.43,0.35 respectively

The decomposition of hydrocarbon follows the equation k=(4.5xx10^11s^-1) e^-28000K/t Calculate E_(a)^(*)