If the rate constant of reaction `k=2times10^(-6)s^(-1)atm^(-1)` . Its value in `dm^(3)mol^(-1)s^(-1)` is

If the rate constant of a reaction is 3.0 mol L^(-1)s^(-1) at 700 K and 30 mol L^(-1)s^(-1) at 800 K, what is the energy of activation for this reaction? R = 8.314 JK^(-1) mol^(-1)

The rate constant of a reaction is 1.5 xx 10^(7)s^(-1) at 50^(@) C and 4.5 xx 10^(7)s^(-1) at 100^(@) C. Calculate the value of activation energy for the reaction (R=8.314 J K^(-1)mol^(-1))

The rate constant for a given reaction is K=3xx10^(-5)S^(-1)" atm"^(-1) . Express it in units of L" mol"^(-1) sec^(-1) .

For the reaction of H_(2) with I_(2) , the constant is 2.5 xx 10^(-4) dm^(3) mol^(-1)s^(-1) at 327^(@)C and 1.0 dm^(3) mol^(-1) s^(-1) at 527^(@)C . The activation energy for the reaction is 1.65 xx 10x J//"mole" . The numerical value of x is __________. (R = 8314JK^(-1) mol^(-1))

The rate constant of a reaction at 300 K is 1.6 xx 10^(-3) sec^(-1) and at 310K it is 3.2 xx 10^(-3) sec^(-1) the activation energy of the reaction approximately in kcals is

At 407 K , the rate constant of a chemical reaction is 9.5xx10^(-5)s^(-1) and at 420 K , the rate constant is 1.9xx10^(-4)s^(-1) . Calculate the Arrhenius parameter of the reaction.

For a reaction, the activation energy is zero. What is the value of rate constant at 300 K if k=1.6 xx 10^(6)s^(-1) at 280 K (R= 8.31 JK^(-1)mol^(-1)) ?