for a reaction activation energy is zero. what is the value of rate constant at 300K, if k=1X`10^(-6)` at 280 K.R=8.314 1) 2X `10^(-6)` `s^(-1)` 2) 4X `10^(-6)` `s^(-1)` 3)1X `10^(-6)` `s^(-1)`

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

For a reaction, activation energy (E_a ) =0 and rate constant, k = 1.5 x 10^4 s^(-1) at 300 K. What is the value of rate constant at 320 K'?

For a reaction the activation energy E_a=0 and the rate constant= 3.2 times 10^6 sec^-1 at 300K. What is the value of rate constant at 310K?

For a decomposition reaction, the values of rate constant k at two different temperatures are given below: K_1 = 2.15 xx 10 ^(-8) L mol^(-1) s^(-1) at 650 K K_2 = 2.39 xx 10^(-7) L mol s^(-1) at 700 K Calculate the value of activation energy for this reaction. (R = 8.314 JK ^(-1) mol^(-1) )

Identify the reaction order form each of the following rate constants: a. k = 7.06 xx 10^(-3) mol L^(-1) s^(-1) b. k = 5.6 xx 10^(-5) s^(-1) c. k = 1.25 xx 10^(-2) mol^(-1)l s^(-1) d. k = 1.25 xx 10^(-2) mol L^(2)s^(-1) e. k = 5.0 xx 10^(-6) atm^(-1)s^(-1)

Identify the reaction order from each of the following rate constants. (i) k = 2.3xx10^(-5)Lmol^(-1)s^(-1) (ii) k = 3xx 10^(-4)s^(-1)