The rate of decomposition of hydrogen peroxide at a particular temperature was measured by titrating its solution with acidic `KMnO_4` solution. Following results were obtained:

Calculate the rate constant ?

The rate of decomposition of hydrogen peroxide at a particular temperature was measured by titrating its solution with acidic KMnO_4 solution. Following results were obtained: Show that the reaction is of first order .

The rate of decomposition of hydrogen peroxide at a particular temperature was measured by titrating its solution with acidic KMnO_4 solution. Following results were obtained : {:("Time t (s)",0,10,20),("Vol. of "KMnO_4"(ml)",11.4,6.9,4.15):} Show that the reaction is of first ordre.

The rate of decomposition of hydrogen peroxide at a particular temperature was measured by titrating its solution with acidic KMnO_4 solution. Following results were obtained. {:("time,t (min)",0,10,20),("Vol. of "KMnO_4"(ml.)",22.8,13.8,8.3):} Show that the reaction is of first order.

The catalytic decomposition of hydrogen peroxide was studied by liberating it at different intervals with KMnO_4 solution. Calculate the rate constant from the following data assuming the reaction to be of the first order :

Compounds ‘A’ and ‘B’ react according to the following chemical equation. A(g) + 2B (g) rarr 2C (g) Concentration of either ‘A’ or ‘B’ were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data is obtained. Calculate the rate constant.

In a pseudo first order hydrolysis of ester in water the following results were obtained: Calculate the pseudo first order rate constant for the hydrolysis of ester.

The decomposition of hydrogen peroxide in the presence of iodide ion has been found to be first order with respect to H_2O_2 with rate constant k is 1.01 xx 10^(-2) min^(-1) . Calculate the rate of reaction when [H_2O_2] = 0.15 mol L^(-1)