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A first order reaction has a half-life of 212 seconds. How long will it take for the concentration of the reactant to decrease to 1/16
- A first order reaction has a half-life of 212 seconds. How long will it take for the concentration of the reactant to decrease to 1/16th of its initial value?
- The data shown were collected for the following first-order reaction: N2O(g) N2(g) + O(g)
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- Use the data to make an Arrhenius plot of lnk vs 1/T. Include the graph when you turn in your homework. (Follow the graphing best practices.)
- What is the equation of the line?
Temperature (K)
Rate constant (1/s)
800.0
0.0000324
900.0
0.00214
1000.0
0.0614
1100.0
0.955
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- What is the activation energy, in kJ, for the reaction? (calculated from the slope)
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