Solution Found!
The rate constant for the second-order reaction is 0.80/M
Chapter 13, Problem 27P(choose chapter or problem)
The rate constant for the second-order reaction
\(2 N O B r(g) \rightarrow 2 N O(g)+B r_{2}(g)\)
is \(0.80 / M \cdot s\) at 10°C. (a) Starting with a concentration of 0.086 M, calculate the concentration of NOBr after 22 s. (b) Calculate the half-lives when \({[N O B r]_{0}}\) = 0.072 M and \({[N O B r]_{0}}\) = 0.054 M.
Questions & Answers
QUESTION:
The rate constant for the second-order reaction
\(2 N O B r(g) \rightarrow 2 N O(g)+B r_{2}(g)\)
is \(0.80 / M \cdot s\) at 10°C. (a) Starting with a concentration of 0.086 M, calculate the concentration of NOBr after 22 s. (b) Calculate the half-lives when \({[N O B r]_{0}}\) = 0.072 M and \({[N O B r]_{0}}\) = 0.054 M.
ANSWER:
Step 1 of 4
We are provided with a second order reaction with a rate constant