Solution Found!

The rate constant for the second-order reaction is 0.80/M

Chapter 13, Problem 27P

(choose chapter or problem)

Get Unlimited 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.

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

Add to cart


Study Tools You Might Need

Not The Solution You Need? Search for Your Answer Here:

×

Login

Login or Sign up for access to all of our study tools and educational content!

Forgot password?
Register Now

×

Register

Sign up for access to all content on our site!

Or login if you already have an account

×

Reset password

If you have an active account we’ll send you an e-mail for password recovery

Or login if you have your password back