Step-by-step explanation:
A. Exothermic .... the Enthalpy of products is less than Enthalpy of reactants
B. For the forward reaction,
A + B --> C + D
∆H(A+B) = 200Kj/mol
∆H(C+D) = 100Kj/mol
∆H = ∆P - ∆R = 100 - 200 = -100KJ/mol
For backward reaction,
C + D ---> A+B
∆H(A+B) = 200Kj/mol
∆H(C+D) = 100Kj/mol
∆H = ∆P - ∆R = 200 - 100 = 100KJ/mol [ Forward is exothermic, backward is endothermic]
C. ... Activated complex should be the peak---that 600kj/mol
D. Activation energies -->
For forward reaction,
Activation energy = (600 - 200) = 400Kj/mol [That's the energy required for the reaction to occur]
For backward reaction, [here, C + D are the reactants ]
Activation energy = (600 - 100) = 500KJ/mol
The forward reaction is to proceed faster because it requires less energy to be overcome, I think.