In a reversible reaction the \(E_{a}\) for the forward and the backward reaction are 50KJ and 30kJ respectively. The value of \(\Delta E\) for the forward reaction is
(A) 20kJ
(B) -20kJ
(C) 80kJ
(D) -80kJ

If the activation energies of the forward and backward reactions of a reversible reaction are E_(a)(f) and E_(a)(b) , respectively. The DeltaE of the reaction is ………..

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4kJ/mol respectively. The reaction is:

The activation energies of the forward and backward reactions in the case of a chemical reaction are 37.5 and 51.3 kJ/mole respectively The reaction is

K_(p) for a reaction at 25^(@)C is 10 atm. The activation energy for forward and reverse reactions are 12 and 20 kJ mol^(-1) respectively. The K_(c) for the reaction at 40^(@)C will be:

The E_a for forward reaction is 50 kcal. The E_a for its backward reaction is:

A colliison between reactant molecules must occur with a certain minimum energy before it is effective in yielding Product molecules. This minimum energy is called activation energy E_(a) Large the value of activation energy, smaller the value of rate constant k . Larger is the value of activation energy, greater is the effect of temperature rise on rate constant k . E_(f) = Activation energy of forward reaction E_(b) = Activation energy of backward reaction Delta H = E_(f) - E_(b) E_(f) = threshold energy In a hypothetical reaction A rarr B , the activation energies for the forward and backward reactions are 15 and 9 kJ mol^(-1) , respectively. The potential energy of A is 10 kJ mol^(-1) . Which of the following is wrong?

In a hypothetical reaction X to Y , the activation energy for the forward backward reactions are 15 and 9 kJ mol^(-1) respectively. The potential energy of X is 10 kJ mol^(-1) . Which of the following statement is/are correct? (i) The threshold energy of the reaction is 25 kJ mol^(-1) (ii) The potential energy of Y is 16 kJ mol^(-1) (iii) Heat of reaction is 6 kJ mol^(-1) The reaction is endothermic.

The activation energy for the forward reaction X rarr Y is 60 kJ mol^(-1) and Delta H is -20 kJ mol^(-1) . The activation energy for the reverse reaction is

For a reaction A rarr B, E_(a) for the forward reaction E_(a(f)) and backward reaction E_(a(b)) is 9kJ mol^(-1) and 9kJ mol^(-1) , respectively. Potential energy of A is 12 kJ mol^(-1) . Calculate (a) The heat of the reaction (b) The threshold energy of reaction (THE)

for a reversible reaction K_(c )gtK_(p) at 298 K and Delta H = + 200 KJ the forward reaction is not favoured by :