Question:
Consider the following reaction in an aqueous solution
\[
\mathrm{I}^-(aq) + \mathrm{OCl}^- \rightarrow \mathrm{IO}^-(aq) + \mathrm{Cl}^-(aq)
\]
and the following initial concentration and initial rate data for this reaction.
Consider the following reaction in an aqueous solution
\[
\mathrm{I}^-(aq) + \mathrm{OCl}^- \rightarrow \mathrm{IO}^-(aq) + \mathrm{Cl}^-(aq)
\]
and the following initial concentration and initial rate data for this reaction.
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Compare experiments where only one reactant concentration changes.
Updated On: Apr 23, 2026
- Rate \(= k [\mathrm{I}^-]^2[\mathrm{OCl}^-]\)
- Rate \(= k[\mathrm{OCl}^-]\)
- Rate \(= k [\mathrm{I}^-]^2\)
- Rate \(= k[\mathrm{I}^-][\mathrm{OCl}^-]\)
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The Correct Option is D
Solution and Explanation
Step 1: Formula / Definition}
\[ \text{Rate} = k[\mathrm{I}^-]^x[\mathrm{OCl}^-]^y \]
Step 2: Calculation / Simplification}
Exp 1 \& 2: \([\mathrm{OCl}^-]\) constant, \([\mathrm{I}^-]\) doubles \(\Rightarrow\) rate doubles \(\Rightarrow x = 1\)
Exp 3 \& 4: \([\mathrm{I}^-]\) constant, \([\mathrm{OCl}^-]\) doubles \(\Rightarrow\) rate doubles \(\Rightarrow y = 1\)
\(\text{Rate} = k[\mathrm{I}^-][\mathrm{OCl}^-]\)
Step 3: Final Answer
\[ \text{Rate} = k[\mathrm{I}^-][\mathrm{OCl}^-] \]
\[ \text{Rate} = k[\mathrm{I}^-]^x[\mathrm{OCl}^-]^y \]
Step 2: Calculation / Simplification}
Exp 1 \& 2: \([\mathrm{OCl}^-]\) constant, \([\mathrm{I}^-]\) doubles \(\Rightarrow\) rate doubles \(\Rightarrow x = 1\)
Exp 3 \& 4: \([\mathrm{I}^-]\) constant, \([\mathrm{OCl}^-]\) doubles \(\Rightarrow\) rate doubles \(\Rightarrow y = 1\)
\(\text{Rate} = k[\mathrm{I}^-][\mathrm{OCl}^-]\)
Step 3: Final Answer
\[ \text{Rate} = k[\mathrm{I}^-][\mathrm{OCl}^-] \]
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