# Hydrogen peroxide and the iodide ion react in acidic solution as follows: H 2 O 2 ( a q ) + 3 I − ( a q ) + 2 H + ( a q ) → I 3 − ( a q ) + 2H 2 O ( l ) The kinetics of this reaction were studied by following the decay of the concentration of H 2 O 2 and constructing plots of ln[H 2 O 2 ] versus time. All the plots were linear and all solutions had [H 2 O 2 ] 0 = 8.0 × 10 −4 mol/L. The slopes of these straight lines depended on the initial concentrations of I − and H + . The results follow: [I − ] 0 (mol/L) [H + ] 0 (mol/L) Slope (min −1 ) 0.1000 0.0400 − 0.120 0.3000 0.0400 − 0.360 0.4000 0.0400 − 0.480 0.0750 0.0200 − 0.0760 0.0750 0.0800 − 0.118 0.0750 0.1600 − 0.174 The rate law for this reaction has the form Rate = − Δ [ H 2 O 2 ] Δ t = ( k 1 + k 2 [ H + ] ) [ I − ] m [ H 2 O 2 ] n a. Specify the order of this reaction with respect to [H 2 O 2 ] and [I − ]. b. Calculate the values of the rate constants, k 1 and k 2 . c. What reason could there be for the two-term dependence of the rate on [H + ]?

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter 11, Problem 112CP
Textbook Problem

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