The reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H20(g) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.) Expt. INO] [H2] Rate, M/sec 1 0.0020 0.0010 0.12 0.0040 0.0010 0.48 3 0.0040 0.0020 0.96 Rate = Calculate the rate constant, k, for the reaction above. (Show work, include units on k.) k =
The reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H20(g) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.) Expt. INO] [H2] Rate, M/sec 1 0.0020 0.0010 0.12 0.0040 0.0010 0.48 3 0.0040 0.0020 0.96 Rate = Calculate the rate constant, k, for the reaction above. (Show work, include units on k.) k =
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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Question
Calculate the rate constant,k, for the reaction about. Show work and include units
Rate= k[No]^2[H2]^1
![The reaction: \(2 \text{NO}(g) + 2 \text{H}_2(g) \rightarrow \text{N}_2(g) + 2 \text{H}_2\text{O}(g)\) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.)
\[
\begin{array}{|c|c|c|c|}
\hline
\text{Expt.} & [\text{NO}] & [\text{H}_2] & \text{Rate, M/sec} \\
\hline
1 & 0.0020 & 0.0010 & 0.12 \\
2 & 0.0040 & 0.0010 & 0.48 \\
3 & 0.0040 & 0.0020 & 0.96 \\
\hline
\end{array}
\]
Rate = _______________
Calculate the rate constant, \(k\), for the reaction above. (Show work, include units on \(k\).)
\(k =\) _______________](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2869a462-41ee-4c15-a1e3-718b6effad40%2F88d88f2e-8ed1-47c5-b0e3-52420fc2bf22%2F0jm1kxd_processed.png&w=3840&q=75)
Transcribed Image Text:The reaction: \(2 \text{NO}(g) + 2 \text{H}_2(g) \rightarrow \text{N}_2(g) + 2 \text{H}_2\text{O}(g)\) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.)
\[
\begin{array}{|c|c|c|c|}
\hline
\text{Expt.} & [\text{NO}] & [\text{H}_2] & \text{Rate, M/sec} \\
\hline
1 & 0.0020 & 0.0010 & 0.12 \\
2 & 0.0040 & 0.0010 & 0.48 \\
3 & 0.0040 & 0.0020 & 0.96 \\
\hline
\end{array}
\]
Rate = _______________
Calculate the rate constant, \(k\), for the reaction above. (Show work, include units on \(k\).)
\(k =\) _______________
Expert Solution
Step 1
Let x and y be the order with respect to [No] & [H2] respectively .
Let us find order of reaction and then calculate the value of rate constant.
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