Solution Found!
The rate constant for the second-order reaction is 0.54/M
Chapter 13, Problem 28P(choose chapter or problem)
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?
Questions & Answers
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 .