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:

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:

For the equilibrium, A(g)rarrB(g), triangleH is - 40 kJ mol^(-1) . If the ratio^f the activation energies of the forward (E_(f)) and reverse (E_(b)) reaction is (2/3) then:

A to B DeltaH =-10KJ mol, E_a=50KJ // mol then activation energy of B to A would be

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

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

For an endothermic reaction, XrarrY . If E_f is activation energy of the forward reaction and E_r that for reverse reaction, which of the following is correct ?