The activation energy for the reaction H₂(g) + I₂(g) $\rightarrow$2HI(g) is changed from 184 kJ/mol to 59.0 kJ/mol at 600. K by the introduction of a Pt catalyst. Calculate the value of the ratio rate(catalyzed)/rate(uncatalyzed).

Question

Quizplus · Accepted Answer

The rate of a reaction is exponentially dependent on the activation energy. Lowering the activation energy from 184 kJ/mol to 59.0 kJ/mol significantly increases the rate. The ratio of the rates can be calculated using the Arrhenius equation, leading to a very large increase, consistent with option D.

The Activation Energy for the Reaction H2(g) + I2(g) →\rightarrow→ 2HI(g) Is Changed from 184 KJ/mol to 59

The Activation Energy for the Reaction H₂(g) + I₂(g) $\rightarrow$ 2HI(g) Is Changed from 184 KJ/mol to 59