In a reaction, the ΔΗ of the reaction was (100 KJ), When a catalyst was used, the activation energy of the reaction decreased by 40 KJ, if the activation energy of forward without catalyst was 280, so the activation energy of the reverse catalytic reaction was…………...

For a one step reaction, the activation energy for the forward reaction is 40.0 kJ mol-1, and the enthalpy of reaction is -20.0 kJ mol-1.  Which statement below is true?Question 2Select one:a.The addition of a catalyst will produce a change in magnitude of the activation energy which is greater for the forward reaction than the reverse reaction.b.The value for the enthalpy of reaction would be decreased by addition of a catalyst.c.The reaction is endothermic.d.The reverse reaction is slower than the forward reaction (smaller rate constant).e.The reaction rate would be decreased by an increase in temperature.

The activation energy for the forward reaction X Y is 60 KJ mol−1 and ΔH is −20 KJ mol−1. The activation energy for the backward reaction Y X is:

Activation energy (E ) and enthalpy of reaction(ΔH) for reaction A → B are 80 kJ mol and–20 KJ mol respectively. On adding catalystactivation energy decreases to 70 KJ mol thenenthalpy of reaction in presence of catalyst is :

Chemistry 121A first order chemical reaction is given as below:A→PAbove reaction is occurring at 500 K. If the same reaction is to be carried out in presence of a catalyst, temperature of 400 K is required, to maintain the same rate of reaction.  If catalyst lowers the activation energy by 30 kJ, then find out value of (t25).(t is value of activation energy of the original pathway (uncatalyzed reaction)) (inkJmole)

A certain catalyzed reaction is known to have an activation energy =Ea50.0/kJmol. Furthermore, the rate of this reaction is measured at 310.K and found to be ×3.8/101Ms. Use this information to answer the questions in the table below.