The following initial rate data were found for the reaction 2MnO4 + 5H2C2O4 + 6H+ → 2 Mn²+ [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is Experiment 1 2 3 4 Rate = K[MnO4]2[H₂C₂O4][H+] Rate = k[MnO4]2[H₂C₂O4]5[H+]6 Rate = k[MnO4]2[H₂C₂O4] Rate = k[MnO4][H₂C2O4][H*] Rate = k[MnO4]²[H₂C₂O4]² [1-] (M) 1.00×10-3 1.00×10-3 2.00×10-3 2.00×10-3 {H+] (M) 1.0 1.0 1.0 2.0 + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6×10-3 1.6×10-3

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The following initial rate data were found for the reaction:

\[ 2\text{MnO}_4^- + 5\text{H}_2\text{C}_2\text{O}_4 + 6\text{H}^+ \rightarrow 2\text{Mn}^{2+} + 10\text{CO}_2 \]

| Experiment | [MnO₄⁻] (M) | [I⁻] (M) | [H⁺] (M) | Rate (M/s)  |
|------------|------------|----------|----------|-------------|
| 1          | 1.00×10⁻³  | 1.00×10⁻³ | 1.0      | 2.0×10⁻⁴   |
| 2          | 2.00×10⁻³  | 1.00×10⁻³ | 1.0      | 8.0×10⁻⁴   |
| 3          | 2.00×10⁻³  | 2.00×10⁻³ | 1.0      | 1.6×10⁻³   |
| 4          | 2.00×10⁻³  | 2.00×10⁻³ | 2.0      | 1.6×10⁻³   |

The rate law for this reaction is:

- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄][H⁺]

- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]⁵[H⁺]⁶

- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]

- ⊗ Rate = k[MnO₄⁻][H₂C₂O₄][H⁺]

- ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]²

This data can be used to determine the appropriate rate law expression for this chemical reaction based on the influence of different initial concentrations on the reaction rate.
Transcribed Image Text:The following initial rate data were found for the reaction: \[ 2\text{MnO}_4^- + 5\text{H}_2\text{C}_2\text{O}_4 + 6\text{H}^+ \rightarrow 2\text{Mn}^{2+} + 10\text{CO}_2 \] | Experiment | [MnO₄⁻] (M) | [I⁻] (M) | [H⁺] (M) | Rate (M/s) | |------------|------------|----------|----------|-------------| | 1 | 1.00×10⁻³ | 1.00×10⁻³ | 1.0 | 2.0×10⁻⁴ | | 2 | 2.00×10⁻³ | 1.00×10⁻³ | 1.0 | 8.0×10⁻⁴ | | 3 | 2.00×10⁻³ | 2.00×10⁻³ | 1.0 | 1.6×10⁻³ | | 4 | 2.00×10⁻³ | 2.00×10⁻³ | 2.0 | 1.6×10⁻³ | The rate law for this reaction is: - ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄][H⁺] - ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]⁵[H⁺]⁶ - ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄] - ⊗ Rate = k[MnO₄⁻][H₂C₂O₄][H⁺] - ⃝ Rate = k[MnO₄⁻]²[H₂C₂O₄]² This data can be used to determine the appropriate rate law expression for this chemical reaction based on the influence of different initial concentrations on the reaction rate.
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