The energy of activation of a reaction is `140 kJ "mol"^(-1)` . If its rate constant at 400 K is `2.0xx10^(-6) s^(-1)`, what is the value at 500 K

The activation energy of a reaction is zero. Its rate constant at 280 K is 16 xx 10^(-6) s^(-1) the rate constant at 300k is

The activation energy of a reaction is 50 kJ mol-1 and the value of rate constant at 300 K is 2.5× 10^-5 sec^-1 . What is the value of the frequency factor, A?

The activation energy of a reaction is 94.14 "kJ mol"^(-1) and the value of rate constant at 313 K is 1.8xx10^(-5) s^(-1) . Calculate the frequency factor A

The activation energy of a reaction is 94.14 kJ mol^(-1) and the value of rate constant at 313 K is 1.8 xx 10^(-5)s^(-1) . Calculate the frequency factor A.

The activation energy of a reaction is 94.14 kJ mol^(-1) and the value of rate constant at 313 K is 18 xx 10^(-5) s^(-1) . Calculate the frequency factor or pre-exponential factor, A .

The activation energy of a reaction is 94.14 "kJ mol"^(-1) and the value of rate constant at 298 K is 18 xx 10^(-5)" s"^(-1) . Calculate the frequency factor or pre-exponential factor, A.

The activation energy of a reaction is 94.14 kJ mol^(-1) and the value of rate constant at 313 K is 18 xx 10^(-5) s^(-1) . Calculate the frequency factor or pre-exponential factor, A .

For a chemical reaction the energy of activation is 85 kJ "mol"^(-1) If the frequency factor is 4.0xx10^(9) L "mol"^(-1)s^(-1) , what is the rate constant at 400 K?