Ask Questions, Get Answers

Want to ask us a question? Click here
Browse Questions
0 votes

A solution of A is mixed with equal volume of a solution of B containing the same number of moles,for reaction $A+B\rightarrow C$.At the end of 1 hour,A is 75% reacted.How much of A will be left unreacted at the end of 2hours if the reaction is first order in A & zero order in B.

$\begin{array}{1 1}(a)\;14.23\%&(b)\;0\%\\(c)\;6.25\%&(d)\;50\%\end{array}$

Can you answer this question?

1 Answer

0 votes
As the given reaction is first order reaction.
$\;\;\;\;=ln 4hr^{-1}$
Now,as K remains constant for a particular reaction,
$K=\large\frac{1}{2hr}$$ln\large\frac{[A_0]}{[A_t]}$$=ln 4hr^{-1}$
$ln\large\frac{[A_0]}{[A_t]}$$=2ln \;4hr^{-1}$
$ln\large\frac{[A_0]}{[A_t]}$$=ln \;16hr^{-1}$
$\large\frac{[A_0]}{[A_t]}$$= \;16$
$\large\frac{[A_t]}{[A_0]}$$= 6.25\%$
answered Dec 18, 2013 by sreemathi.v
edited Jul 27, 2014 by balaji.thirumalai

Related questions

Ask Question
student study plans
JEE MAIN, CBSE, NEET Mobile and Tablet App
The ultimate mobile app to help you crack your examinations
Get the Android App