Determine the order of reaction with respect to \( H_2O_2 \), \( I^- \) and overall order of reaction.
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Solution and Explanation
• The order of reaction with respect to a specific reactant is the exponent to which its concentration is raised in the rate law.
• The overall order is the sum of the individual orders of all reactants in the rate law.
Step 1: Extract individual orders from the rate law
From the rate law \( \text{Rate} = k [H_2O_2]^1 [I^-]^1 \):
The exponent for \( [H_2O_2] \) is 1.
The exponent for \( [I^-] \) is 1.
Step 2: Calculate the overall order
Overall order \( = \text{Order wrt } H_2O_2 + \text{Order wrt } I^- \)
Overall order \( = 1 + 1 = 2 \). The final answer is Order wrt \( H_2O_2 = 1 \), \( I^- = 1 \), Overall order \( = 2 \).
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