For the Equillibrium `A(g) hArr B(g)`, `DeltaH` = -42KJ/mol if the ratio of the activation energy of forward & backward reaction is `2/3` then find `E_f`and `E_b`

For the equilibrium, A(g)hArrB(g),DeltaH is -40kJ//mol , if the ratio of the activation energies of the forward (E_(f)) and reverse (E_(b)) reactions is 2/3, then

For the equilibrium, A(g) rarr B(g) , DeltaH is -40 KJ/mol. If the ratio of the activation energies of the forward (E_(f)) and reverse (E_(b)) reactions is (2)/(3) then:

A+B rarr C, DeltaH = +60 kJ/mol E_(a_f) is 150 kJ. What is the activation energy for the backward reaction ?

If E_(f) and E_(r) are the activation energies of forward and backward reactions and the reaction is known to be exothermic, then

For a hypothetical reaction, 2A+B hArr C + energy , the activeation energy of forward reaction (E_(af)) and backward reaction (E_(ab)) are related as

For A+B rarr C+D, DeltaH=-20 kJ mol^(-1) , the activation energy of the forward reaction is 85 kJ mol^(-1) . The activation energy for backward reaction is …… kJ mol^(-1) .

For A + B to C + D, DeltaH = -20 kJ "mole"^(-1) . The activation energy for the forward reaction is 85 kJ. Then the activation energy for the backward reaction is ___

The energy change accompanying the equilibrium reaction A hArr B is -33.0 kJ mol^(-1) . Assuming that pre-exponential factor is same for forward and backward reaction answer the following: The energy of activation for forward and backward reactions ( E_(f) and E_(b) ) at 300 K . Given that E_(f) and E_(b) are in the ratio 20 : 31 ,