Question

For a reaction $A_{2} + B_{2}$2AB the figures shows the path of the reaction in absence and presence of a catalyst. What will be the energy of activation for forward $(E_{f})$ and backward $(E_{b})$ reaction in presence of a catalyst and $\Delta H$ for the reaction? The dotted curve is the path of reaction in presence of a catalyst.

• A. $E_{f} = 60kJ/mol,E_{b} = 70KJ/mol,\Delta H = 20KJ/mol$
• B. $E_{f} = 20kJ/mol,E_{b} = 20KJ/mol,\Delta H = 50KJ/mol$
• C. $E_{f} = 70kJ/mol,E_{b} = 20KJ/mol,\Delta H = 10KJ/mol$
• D. $E_{f} = 10kJ/mol,E_{b} = 20KJ/mol,\Delta H = - 10KJ/mol$

Answer 1

Answer: (D)

$E_{f} = 10kJ/mol,E_{b} = 20KJ/mol,\Delta H = - 10KJ/mol$

Answer 2

$E_{f} = 70 - 60 = 10kJ/mol$

$E_{b} = 70 - 50 = 20kJ/mol$

$\Delta H = 50 - 60 = - 10kJ/mol$