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 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) :

Aqueous AB_(2) decomposes according to the first order reaction: AB_(2)(aq) rarr A(g) + 2B(l) After 20 min the volume of A(g) colledcted during such a reaction is 20 mL , and that collected after a very long time is 40 mL . The rate constant is :

For a reaction,\(A \rightarrow products\), rate increases x times when concentration of 'A' increases y' times, then order of reaction 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 compoistion of N_(2)O_(5) is a first order reaction represented by: N_(2)O_(5) rarr N_(2)O_(4) + 1//2O_(2) . After 20 min the volume of O_(2) profuced is 10 mL and at the end of the reaction 40 mL . The rate constant is equal to

Show that for the reactions of first order (i) Half-life period is independent of initial concentrations. (ii) Units of rate constant do not depend upon the units of concentration.

Reaction \(P\rightarrow Q\).The half-life of the reaction and concentration of "P" is given in graph Concentration of P decreases from "1M" to "0.25M" in "100" minutes, the initial rate of reaction (in M/minute)

The decomposition of N_2O_5 is a first order reaction represented by : N_2O_5 to N_2O_4 + ½O_2 . After 15 minutes the volume of O_2 produced is 9 ml and at the end of the reaction is 35 ml. The rate constant given by the expression: