- #1

- 6

- 0

## Homework Statement

The second-order rate constant for the reaction A+2B --> 2C+D is 0.34 dm

^{3}/mol s. What is the concentration of C after 20 s and 15 min if the initial concentrations were [A] = 0.027 mol/dm

^{3}and [ B] = 0.130 mol/dm

^{3}

## Homework Equations

The integrated rate law for A+2B --> P

$$k_r t=\frac{1}{[B ]_0-2[A]_0}\ln\frac{[A]_0([B ]_0-2x)}{([A]_0-x)[B ]_0}$$

with $$x=[P]$$ as it is given in Physical Chemistry by Atkins.

## The Attempt at a Solution

Solving the above equation for x gives

$$x=\frac{[ B](\exp(k_r t([ B]-2[A]))-1)}{\frac{[ B]}{[A]}\exp(k_r t([ B]-2[A]))-2}.$$

By inserting the numbers from the problem statement I get x = 0.014485 mol/dm

^{3}.

But I can't really figure out if [C] is just 2/3 *x, since we have 2C and 1D as the products or what the final answer is.

thanks