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.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![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.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F18593a3a-b463-4aeb-a821-a472ffee6b36%2F37cfb881-4ebc-42d2-8ea1-532f79627f10%2F5jrmox4_processed.png&w=3840&q=75)
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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