**Question 18**For the reaction below, we are told the overall rate order = 3.\[ 3 \: \text{I}^- \, (\text{aq}) + \text{H}_3\text{AsO}_4 \, (\text{aq}) + 2 \: \text{H}^+ \, (\text{aq}) \rightarrow \text{I}_3^- \, (\text{aq}) + \text{H}_3\text{AsO}_3 \, (\text{aq}) + \text{H}_2\text{O} \, (\text{l}) \]**Which of the following is the correct rate law?**- $\text{Rate} = k[\text{I}^-]^2[\text{H}_3\text{AsO}_4][\text{H}^+]^{-1}$- $\text{Rate} = k[\text{I}^-]^2[\text{H}_3\text{AsO}_4][\text{H}^+]$- $\text{Rate} = k[\text{I}^-]^2[\text{H}_3\text{AsO}_4]$- $\text{Rate} = k[\text{I}^-]^3[\text{H}_3\text{AsO}_4][\text{H}^+]^2$- $\text{Rate} = k[\text{I}^-]^2[\text{H}_3\text{AsO}_4]^2$*A reminder: Moving to another question will save this response.*

The balanced reaction is – 3I-aq+H3AsO4aq+ 2H+aq →I3-aq +H3AsO3aq + H2Ol

Answered: **Question 18** For the reaction…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Expert Solution

Step 1

The balanced reaction is –

$3 I^{-} (aq) + H_{3} {AsO}_{4} (aq) + 2 H^{+} (aq) \to {I_{3}}^{-} (aq) + H_{3} {AsO}_{3} (aq) + H_{2} O (l)$

Step 2

Order of the reaction is given = 3

Order is obtained by addition of powers of concentration mentioned in the rate law.

$\begin{array}{rcl} (a) Rate & = & k {[I^{-}]}^{2} {[H_{3} {AsO}_{4}]}^{2} {[H^{+}]}^{- 1} \\ order & = & 2 + 2 + (- 1) = 3 \\ (b) Rate & = & k {[I^{-}]}^{2} [H_{3} {AsO}_{4}] [H^{+}] \\ order & = & 2 + 1 + 1 = 4 \\ (c) Rate & = & k {[I^{-}]}^{2} [H_{3} {AsO}_{4}] [H^{+}] \\ order & = & 2 + 1 + 1 = 4 \end{array}$