1. Tardigrade
  2. Question
  3. Chemistry
  4. The energies of activation for forward and reverse reactions for A2 + B2<=>2AB are 180 kJ mol−1 and 200 kJ mol−1 respectively. The presence of catalyst lowers the activation energy of both (forward and reverse) reactions by 100 kJ mol−1. The enthalpy change of the reaction (A2 + B2->2AB) in the presence of catalyst will be (in kJ mol−1)

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. The energies of activation for forward and reverse reactions for $\ce{A2 + B2<=>2AB}$ are $180\, kJ \,mol^{−1}$ and $200\, kJ\, mol^{−1}$ respectively. The presence of catalyst lowers the activation energy of both (forward and reverse) reactions by $100\, kJ\, mol^{−1}$. The enthalpy change of the reaction ($\ce{A2 + B2->2AB}$) in the presence of catalyst will be (in $kJ\, mol^{−1}$)

AIEEEAIEEE 2007Chemical Kinetics

Solution:

So, $\Delta H_{Reaction}=E_{f}-E_{b}$
$= 80 - 100 = -20$
Hence, $\left(4\right)$ is correct.

Solution Image