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The data of the initial rate experiment of the following reaction are given below. The rate law expression of the reaction is Rate = k[S208 J*[ r}Y. Determine the rate constant k with 3 significant figures (key-in only your value; no units are needed). Note that your k value should be reported based on second (the time units here). Do not covert second to other time units. S208° (aq) + 3 I" (aq) → 2 so4²" (aq) + 13` (aq) (S20g Jo (M) [rJo (M) initial rate (M/sec) Trial 1 0.800 0.140 0.0288 Trial 2 2.400 0.140 0.2592 Trial 3 0.800 0.280 0.0288 Note that Trial 1 and Trial 3 have the same initial rate.

The data of the initial rate experiment of the following reaction are given below. The rate law expression of the reaction is Rate = k[S208 J*[ r}Y. Determine the rate constant k with 3 significant figures (key-in only your value; no units are needed). Note that your k value should be reported based on second (the time units here). Do not covert second to other time units. S208° (aq) + 3 I" (aq) → 2 so4²" (aq) + 13` (aq) (S20g Jo (M) [rJo (M) initial rate (M/sec) Trial 1 0.800 0.140 0.0288 Trial 2 2.400 0.140 0.2592 Trial 3 0.800 0.280 0.0288 Note that Trial 1 and Trial 3 have the same initial rate.

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The data of the initial rate experiment of the following reaction are given below. The rate law expression of the reaction is Rate = \( k \ [ \text{S}_2\text{O}_8^{2-} ]^x [ \text{I}^- ]^y \). Determine the rate constant \( k \) with 3 significant figures (key in only your value; no units are needed). Note that your \( k \) value should be reported based on second (the time units here). Do not convert second to other time units. \[ \text{S}_2\text{O}_8^{2-} (\text{aq}) + 3 \, \text{I}^- (\text{aq}) \rightarrow 2 \, \text{SO}_4^{2-} (\text{aq}) + \text{I}_3^- (\text{aq}) \] \[ \begin{array}{|c|c|c|c|} \hline \text{Trial} & [\text{S}_2\text{O}_8]_{0} \, (\text{M}) & [\text{I}^-]_{0} \, (\text{M}) & \text{Initial rate} \, (\text{M/sec}) \\ \hline 1 & 0.800 & 0.140 & 0.0288 \\ 2 & 2.400 & 0.140 & 0.2592 \\ 3 & 0.800 & 0.280 & 0.0288 \\ \hline \end{array} \] **Note that Trial 1 and Trial 3 have the same initial rate.**
Transcribed Image Text:The data of the initial rate experiment of the following reaction are given below. The rate law expression of the reaction is Rate = \( k \ [ \text{S}_2\text{O}_8^{2-} ]^x [ \text{I}^- ]^y \). Determine the rate constant \( k \) with 3 significant figures (key in only your value; no units are needed). Note that your \( k \) value should be reported based on second (the time units here). Do not convert second to other time units. \[ \text{S}_2\text{O}_8^{2-} (\text{aq}) + 3 \, \text{I}^- (\text{aq}) \rightarrow 2 \, \text{SO}_4^{2-} (\text{aq}) + \text{I}_3^- (\text{aq}) \] \[ \begin{array}{|c|c|c|c|} \hline \text{Trial} & [\text{S}_2\text{O}_8]_{0} \, (\text{M}) & [\text{I}^-]_{0} \, (\text{M}) & \text{Initial rate} \, (\text{M/sec}) \\ \hline 1 & 0.800 & 0.140 & 0.0288 \\ 2 & 2.400 & 0.140 & 0.2592 \\ 3 & 0.800 & 0.280 & 0.0288 \\ \hline \end{array} \] **Note that Trial 1 and Trial 3 have the same initial rate.**
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