Multiple Choice
Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I⁻(aq). What is the rate law for this reaction?
15. Chemical Kinetics
Intro to Chemical Kinetics
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In the reaction 3 BrO⁻(aq) → BrO₃⁻(aq) + 2 Br⁻(aq), a plot of 1/[BrO⁻] vs. time is linear. What does this indicate about the order of the reaction with respect to BrO⁻?
A
Third order
B
Zero order
C
First order
D
Second order
Verified step by step guidance1
Understand the relationship between the plot and reaction order: A linear plot of 1/[Reactant] vs. time indicates a second-order reaction with respect to that reactant.
Recall the integrated rate law for a second-order reaction: The integrated rate law for a second-order reaction is \( \frac{1}{[A]} = kt + \frac{1}{[A_0]} \), where \([A]\) is the concentration of the reactant, \(k\) is the rate constant, \(t\) is time, and \([A_0]\) is the initial concentration.
Identify the reactant in the given reaction: The reactant in the given reaction is \( \text{BrO}^- \).
Relate the plot to the integrated rate law: Since the plot of \( \frac{1}{[\text{BrO}^-]} \) vs. time is linear, it matches the form of the second-order integrated rate law, confirming the reaction is second order with respect to \( \text{BrO}^- \).
Conclude the order of the reaction: Based on the linear plot of \( \frac{1}{[\text{BrO}^-]} \) vs. time, the reaction is second order with respect to \( \text{BrO}^- \).
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