Question

The reaction between H$_2$ (g) and I$_2$ (g) was carried out in a sealed isothermal chamber. The rate law for the reaction was found to be: \[ \text{Rate} = k[\text{H}_2][\text{I}_2] \] If 1 mole of H$_2$ (g) was added to the reaction chamber and the temperature was kept constant, then predict the change in rate of the reaction and the rate constant.

Hint:

For reactions with multiple reactants, changes in the concentration of one reactant will proportionally affect the reaction rate, depending on the order of reaction.

Answer 1

For a second-order reaction involving H$_2$ and I$_2$, the reaction rate is directly proportional to the product of their respective concentrations.
If 1 mole of H$_2$ is added while the I$_2$ concentration is held constant, the reaction rate will increase proportionally to the augmented H$_2$ concentration.
As the temperature is constant, the rate constant (k) remains invariant.
Consequently, an increase in H$_2$ concentration leads to a higher reaction rate.