In a first order reaction The initial concentration of [A] = 0.3 mol/lit. The concentration after 2.3 min is 0.15 moles/lit. What is the value of rate constant.

For a zero order reaction '[R]_0 is the initial concentration

The half life of a first order reaction is 10 minutes. If initial amount is 0.08 mole/litre and concentration at some instant ‘t’ is 0.01 mol/litre, then the value of ‘t’ is :

For the reaction , Cl_(2)+2I^(-) rarr I_(2)+2Cl^(-) , the initial concentration of I^(-) was 0.20 "mol lit"^(-1) and the concentration after 20 minutes was 0.18 "mol lit"^(-1) . Then the rate of formation of I_(2) in "mol lit"^-1min^-1 would be

The rate constant of a first order reaction is proportional to the concentration of the reactant.

A subtance 'A' decomposes by a first-order reaction starting initially with [A] = 2.00 m and after 200 min [A] = 0.15 m . For this reaction what is the value of k

In a first-order reaction A→B, if k is rate constant and initial concentration of the reactant A is 0.5 M then the half-life is:

In a first-order reaction A rarr B , if K is the rate constant and initial concentration of the reactant is 0.5 M , then half-life is

In a first order reaction, the concentration of the reactant decreases form 0.8 M to 0.4 M in 15 min . The time taken for the concentration to change form 0.1 M to 0.025 M is