The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 Rate k = AsO3³+ 2Ce4+. = 4+ [ASO3³] [C¹+] M M 0.0311 0.0622 0.0311 0.0622 3- + H₂O → AsO4³ + 2Ce³+ + 2H+ M-2.s -1 0 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. I 0.145 0.145 0.290 0.290 Initial Rate, -1 M.s 0.000345 0.000690 0.00138 0.00276
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 Rate k = AsO3³+ 2Ce4+. = 4+ [ASO3³] [C¹+] M M 0.0311 0.0622 0.0311 0.0622 3- + H₂O → AsO4³ + 2Ce³+ + 2H+ M-2.s -1 0 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. I 0.145 0.145 0.290 0.290 Initial Rate, -1 M.s 0.000345 0.000690 0.00138 0.00276
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.101PAE
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![The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:
\[ \text{AsO}_3^{3-} + 2 \text{Ce}^{4+} + \text{H}_2\text{O} \rightarrow \text{AsO}_4^{3-} + 2 \text{Ce}^{3+} + 2 \text{H}^+ \]
| Experiment | \([\text{AsO}_3^{3-}]_0\), M | \([\text{Ce}^{4+}]_0\), M | Initial Rate, M·s\(^{-1}\) |
|------------|----------------------|---------------------|-------------------------------|
| 1 | 0.0311 | 0.145 | 0.000345 |
| 2 | 0.0622 | 0.145 | 0.000690 |
| 3 | 0.0311 | 0.290 | 0.00138 |
| 4 | 0.0622 | 0.290 | 0.00276 |
Complete the rate law for this reaction in the box below.
Use the form \(k[\text{A}]^m[\text{B}]^n\), where '1' is understood for \(m\) or \(n\) and concentrations taken to the zero power do not appear. Don't enter 1 for \(m\) or \(n\).
Rate = \_\_\_\_
\[ k = \_\_\_\_ \text{ M}^{-2} \cdot \text{s}^{-1} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e780e57-9ac3-4969-b842-a86b4366ba1d%2Fd5aa0fa4-5ce9-4232-9198-07a084fe96bc%2F0evnyhe_processed.png&w=3840&q=75)
Transcribed Image Text:The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution:
\[ \text{AsO}_3^{3-} + 2 \text{Ce}^{4+} + \text{H}_2\text{O} \rightarrow \text{AsO}_4^{3-} + 2 \text{Ce}^{3+} + 2 \text{H}^+ \]
| Experiment | \([\text{AsO}_3^{3-}]_0\), M | \([\text{Ce}^{4+}]_0\), M | Initial Rate, M·s\(^{-1}\) |
|------------|----------------------|---------------------|-------------------------------|
| 1 | 0.0311 | 0.145 | 0.000345 |
| 2 | 0.0622 | 0.145 | 0.000690 |
| 3 | 0.0311 | 0.290 | 0.00138 |
| 4 | 0.0622 | 0.290 | 0.00276 |
Complete the rate law for this reaction in the box below.
Use the form \(k[\text{A}]^m[\text{B}]^n\), where '1' is understood for \(m\) or \(n\) and concentrations taken to the zero power do not appear. Don't enter 1 for \(m\) or \(n\).
Rate = \_\_\_\_
\[ k = \_\_\_\_ \text{ M}^{-2} \cdot \text{s}^{-1} \]
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