- #1
hedegaardo1
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Homework Statement
The second-order rate constant for the reaction A+2B --> 2C+D is 0.34 dm3/mol s. What is the concentration of C after 20 s and 15 min if the initial concentrations were [A] = 0.027 mol/dm3 and [ B] = 0.130 mol/dm3
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/dm3.
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