Ask Questions, Get Answers

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

A compound exists in the gaseous phase both as monomer (A) and dimer $(A_2)$. The molecular weight of A is 48 . In an experiment 96g of the compound was confined in a vessel of volume 33.6 litre and heated to $273^{\large\circ}C$. Calculate the pressure developed if the compound exists as dimer to the extent of $50\%$ by weight under these conditions.


Can you answer this question?

1 Answer

0 votes
since A and $A_2$ are two states in gaseous phase having their weight ratio$50\%$ i.e 1:1
$\therefore Mole\;of\;A = \large\frac{96}{2}\times\large\frac{1}{48} = 1$
We have n =$ \large\frac{w}{m}$
$\therefore Mole\;of\;A_2 = \large\frac{96}{2}\times\large\frac{1}{96} = \large\frac{1}{2}$
$\therefore Total\;mole\;of\;A and A_2 are = 1+\large\frac{1}{2} = \large\frac{3}{2}$
We know that PV = nRT
$P\times33.6 = \large\frac{3}{2}\times0.0821\times546$
P = 2 atm
Hence answer is (c)
answered Feb 15, 2014 by sharmaaparna1

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