In general, it is observed that the rate of a chemical reaction doubles with every `10^(@)` rise in temperature. If the generalisation holds for a reaction in the temperature range 295 K to 305 K, what would be the value of activation energy for the reaction?

In general it is observed that the rate of a chemical reaction doubles with every 10^@ rise in temperature. If the generalisation holds for a reaction in the temperature range 295K to 305K, what would be the value of activation energy for the reaction?

In general, it is observed that the rate of a chemical reaction doubles with every 10° rise in temperature. If this generalisation holds for a reaction in the temperature range 298 K to 308 K, what would be the value of activation energy for this reaction ? (R = 8.314 JK^(-1) mol^(-1) )

In general it is observed that the rate of a chemical reaction doubles with every 10^(circ) rise in temperature. If this generalisation holds for a reaction in the temperature range 295 (~K) to 305 (~K) , what would be the value of activation energy for this reaction? (R)=8.314 (Jk)^(-1) (~mol)^(-1)

In general it is observed that the rate of a chemical reaction doubles with every 10 degree rise in temperature. If the generalization holds good for the reaction in the temperature range 295 K to 305 K, what would be the value of activation energy for this reaction ? [R = 8.314 mol^(-1)JK^(-1)]

In general it is observed that the rate of a chemical reaction becomes double for every 10^@ rise in temperature. If this generalisation holds for a reaction in the temperature range 2908 K to 398 K, what would be the value of activation energy for the reaction. (R=8.314 J K^(-1)mol^(-1) )

The rate of a chemical reaction becomes double for every 10^@C rise in temperature. If this generalisation holds for a reaction in the temperature range 290 K to 300 K, what would be the approximate value of E_a for the reaction ?