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The rate constant for the second-order reaction is 0.54/M

Chapter 13, Problem 28P

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QUESTION:

The rate constant for the second-order reaction

\(2 \mathrm{NO}_{2}(g) \rightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)

is \(0.54 / M \cdot s\) at 300°C. How long (in seconds) would it take for the concentration of \(\mathrm{NO}_{2}\) to decrease from 0.62 M to 0.28 M?

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QUESTION:

The rate constant for the second-order reaction

\(2 \mathrm{NO}_{2}(g) \rightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)

is \(0.54 / M \cdot s\) at 300°C. How long (in seconds) would it take for the concentration of \(\mathrm{NO}_{2}\) to decrease from 0.62 M to 0.28 M?

ANSWER:

Step 1 of 4

Given data

The rate constant of the reaction is .

The initial concentration of reactant .

*The final concentration of a reactant at time t is .

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