A plot of `"Ink "v//s " 1/T"` for a reaction gives the slope `-1xx10^(4)k.` The energy of activation for the reaction is `(Given,R=8.314k^(-1)" mol"^(-1))`

The slope of Arrhenius plot (l_(n)k " vs " 1//J) of a first order reaction is -5 xx 10^(3) . The value of E_(a) of the reaction is (R = 8.314 J K^(-1)mol^(-1))

The rate of a reaction triples when temperature changes from 50 to 100^(@)C. Calculate the energy of activation for such a reaction (R=8.314" J K"^(-1)" mol"^(-1))

The slope of a line in the graph of log k versus 1/T for a reaction is -5841 K. Calculate energy of activation for the reaction.

Rate constant k of a reaction varies with temperature according to the equation logk=" constant"-(E_(a))/(2.303).(1)/(T) where E_(a) is the energy of activation for the reaction. When a graph is plotted for log k versus 1//T , a straight line with a slope -6670 K is obtained. Calculate the energy of activation for this reaction. State the units (R=8.314" JK"^(-1)mol^(-1))

The reaction C_(2)H_(5)I to C_(2)H_(4) + HI is of first order and its rate constants are 3.20 xx 10^(-4) s^(-1) at 600 K and 1.60 xx 10^(-2)s^(-1) at 1200 K. Calculate the energy of activation for the reaction. (Given R= 8.314 JK^(-1)mol^(-1))

The slope of Arrhenius Plot (lnK v/s 1/T) of 1st order reaction is -5x 10^3 K. The value of E_a of the reaction is.

The rate constant for a reaction is 2xx10^(-2) s^(-1) at 300 K and 8xx10^(-2) s ^(-1) at 340 K The energy of activation of the reaction is