Physical Chemistry

two flask of equal voliume connected by a narrow tube (of negligible volume) are at 27C and contains 0.7 moles of H2 at 0.5 atm .one of the flask is then immersed in a bath kept at 127C while the other reains at 27C .calculate the final pressure and the number of moles of H2 in each flask

krishnan s

15 Years agoGrade

4 Answers

saurabh av

Approved Tutor Answer15 Years ago

PV=nRT

0.5v=0.7R300

so v=420R

In 2nd case the pressure will be same in both flasks and sum of moles of gas will be 0.7

Flask 1-

PV=aRT

P420R=aR300

a=1.4P

Flask2-

PV=bRT

P420R=bR400

b=1.05P

a + b = 2.45P = 0.7

P = 0.28

a= 0.294, b= 0.392

meetakshi behal

14 Years ago

why did u take volume of both the flasks in case2 same..?

i mean if the volume of two flasks together is 420R, the the volume of 1 flask shud have been 210.

Aadi

9 Years ago

The volumes does not depict volume of container but gas.In expression PV=nRT V is volume of gas taken.Thus taking 420R in this case is valid.

ankit singh

5 Years ago

Two flasks of equal volume connected by a narrow tube (of negligible volume) are at 27∘C and contain 0.70 mole of H2 to 0.5atm One of the flask is then immersed into a bath kept at 127∘C while the other remains at 27∘C Calculate the final pressure and the number of mole of H2 in each flask .