Ask Questions, Get Answers

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

For the reaction ,$N_2O_5(g)\iff 2NO_2(g)+0.5O_2(g)$.Calculate the mole fraction of $N_2O_5(g)$ decomposed at a constant volume and temperature,if the initial pressure at any time is 960mm Hg.Assume ideal gas behaviour.


Can you answer this question?

1 Answer

0 votes
$N_2O_5\iff 2NO(g)+\large\frac{1}{2}$$O_2$(g)
Initial pressure :
$N_2O_5\Rightarrow 600$
$2NO\Rightarrow 0$
$\large\frac{1}{2}$$O_2\Rightarrow 0$
Final pressure :
$2NO\Rightarrow 600-p$
$2p\Rightarrow 2p$
$\large\frac{1}{2}$$O_2\Rightarrow \large\frac{p}{2}$
Step 2:
$p\alpha$ moles if $V,T$ are constant.
$\therefore 600-p+2p+\large\frac{p}{2}$$=960$
$\therefore$ Mole fraction Of $N_2O_5$ decomposed $=\large\frac{240}{600}$
$\Rightarrow 0.4$
Hence (d) is the correct answer.
answered Nov 6, 2013 by sreemathi.v

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