Half life id independent of the concentration of `A`. After `10 mi n` volume of `N_(2)` gas is `10 L` and after complete reaction is `50 L`. Hence, the rate constant is

Half- life is independent of conc. of A. After 10 minutes volume N_(2) gas is 10 L and after complete reaction 50 L. Hence rate constant in "min"^(–1) :

For reaction \(X \rightarrow Y+Z\) half life is independent of the concentration of X. After "20" minutes volume of gas "Z" is "10mL and after very long time it is "50mL" ,the rate constant is

For reaction X rarr Y+Z half life is independent of the concentration of X .After 20 minutes volume of gas Z is 10mL and after very long time it is 50mL ,the rate constant is : 1) (2.303)/(20)log5 2) (2.303)/(20)log1.25 3) (2.303)/(10)log2 4) (2.303)/(20)log4

Half life of reaction : H_(2)O_(2)(aq) rarr H_(2)O(l)+(1)/(2)O_(2)(g) is independent of initial concentration of H_(2)O_(2) volume of O_(2) gas after 20 minute is 5L at 1 atm and 27^(@)C and after completion of reaction is 50L . The rate constant is :

Half life of reaction : H_(2)O_(2)(aq) rarr H_(2)O(l)+(1)/(2)O_(2)(g) is independent of initial concentration of H_(2)O_(2) volume of O_(2) gas after 20 minute is 5L at 1 atm and 27^(@)C and after completion of reaction is 50L . The rate constant is :

The initial concentration of the reactant in a zero order reaction is 1.386 "mol.L"^(-1) The half-life of the reaction is 20s. Calculate: the rate constant

Benzene diazonium chloride (A) decoposes into chlorobenzene (B) and N_(2) (g) in first order reaction. Volumes of N_(2) collected after 5 min and at the complete decomposition of A are 10 mL. and 50mL respectively. The are constant for the reaction is

(A) Half-life period is always independent of initial concentration. (R ) Half-life period is inversely proportional to rate constant.

The rate of a first order reaction is 1.8 xx10^-3 mol L^-1 mi n^-1 when the initial concentration is 0.3 mol L^-1 . The rate constant in the units of second is :