The rate constant of a reaction with respect to the reactant A is `6min^-1`. If we start with `[A] = 0.8mol L^-1`, when would [A] reach the value of 0.08 mol L^-1?

The rate constant of a reaction is 3xx10^2 min^-1 . What is the order of the reaction?

The rate constant for the decomposition of a hydrocarbon is 2.418xx10^-5 s^-1 at 546 K. If the energy of activation is 179.9 KJ mol^-1 , What will be the value of pre-exponential factor?

For the reaction: 2A + B rarr A_2B the rate = k[A][B]^2 with k = 2.0xx10^-6 mol^-2 L^2 s^-1 . Calculate the initial rate of the reaction when [A] = 0.1 mol L^-1 , [b] = 0.2 mol L^-1 . Calculate the rate of reaction after [A] is reduced to 0.06 mol L^-1 .

What is meant by the 'rate constant, k' of a reaction. If the concentration be expressed in mol L^1 units and time in seconds, what would be the units for k for a zero order reaction and for a first order reaction.

The rate constant for the decomposition of hydrocarbons is 2.418xx10^(-5)s^(-1) at 546K. If the energy of activation is 179.9kJ//mol what will be the value of pre-exponantial factor?

The rate of a reaction is 1.2xx10^-3 L mol^-1 s^-1 . What is the order of the reaction?

A reaction is second order with respect to a reacant. How is the rate of reaction affected if the concentration of the reactant is reduced to 1/2?

The rate constant for a first order reaction is 60s^-1 . How much time will it take to reduce the concentration of the reactant to 1//16^(th) of its initial value?

The rate constant for a first order reaction is 60s^-1 . How much time will it take to reduce the concentration of the reactant to 1//16^(th) of its initial value?

The rate constant of a reaction at 500K and 700K are 0.01s^-1 and 0.07s^-1 respectively. Calculate the value of activation energy for the reaction (R = 8.314 JK^-1mol^-1).