Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: KaczuH on August 01, 2011, 08:17:20 AM
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I've tried solving it but I'm not even close to the answer. Please confirm my doubts or give a hint how to calculate the problem.
$$ O_{3} + NO \rightarrow NO_{2} + O_{2} /$$
Rate equation
$$ v=k[O_{3}][NO] /$$
Concetrations:
$$ [O_{3}] = 2.04*10^{-5} M /$$
$$ [NO] = 5*10^{-5} M /$$
$$ k = 3*10^{6} \frac{1}{M*s} /$$
How many moles of NO2 is in volume of 1dm3 after one hour?
The answer is 10.8 moles of NO2, but if we consider concentration of ozone it is impossible, because of conserwation of mass.
My solution:
$$ v=\frac{dC_{NO_{2}}}{dt}=\frac{dx}{dt}=k([O_{3}]_{0}-x)([NO]_{0}-x) /$$
After integration
$$ kt([NO]_{0}-[O_{3}]_{0})=ln(\frac{([NO]_{0}-x)*[O_{3}]_{0}}{([O_{3}]_{0}-x)[NO]_{0}}) /$$
What is wrong?