For given reaction`A to Products`, rate constant 'K' for the reaction is `0.6 mol L^(-1) min^(-1)`. If initial concentration of reactant A is 8 mol/L , concentration of A after 10 minutes will be:

For a zero order reaction, K=1xx10^(-3)"mol L"^(-1)s^(-1) If initial concentration of the reactant is 1.0"mol L"^(-1) , the concentration after 10 minutes would be

The specific rate constant for a first order reaction is 60xx10^(-4) sec^(-1) . If the initial concentration of the reactant is 0.01mol L^(-1) , the rate is

For a particular reaction (A rightarrow B) the rate constant is 0.693 (min)^-1 If the initial concentration of the reactant, A is 1 M, then the rate of reaction after 1 minute will be

The rate constant for a zero order reaction is 2xx10^(-2) mol L^(-1) sec^(-1) . If the concentration of the reactant after 25 sec is 0.5 M , the initial concentration must have been:

Rate constant k=2.303 min^(-1) for a particular reaction. The initial concentration of the reactant is 1 mol // litre then rate of reaction after 1 minute is:

The rate for a first order reaction is 0.6932 xx 10^(-2) mol L^(-1) "min"^(-1) and the initial concentration of the reactants is 1M , T_(1//2) is equal to

The rate for a first order reaction is 0.6932 xx 10^(-2) mol L^(-1) "min"^(-1) and the initial concentration of the reactants is 1M , T_(1//2) is equal to

The rate constant of the reaction A rarr 2B is 1.0 xx 10^(-3) mol "lit" ^(-1)" min"^(-1) , if the initial concentration of A is 1.0 mole lit^(-1) . What would be the concentration of B after 100 minutes.

The rate of first order reaction is 1.5 xx 10^(-2) mol L^(-1) min ^(-1) at 0.5 M concentration of the reactant. The half-life of the reaction is