Two flasks of equal volume are connected by a narrow tube (of negligible volume) all at 27ºC and contain 0.70 mole of H2 at 0.5 atm. One of the flask is then immersed into a bath kept at 127 
C, while the other remains at 27 
C. The final pressure in each flask is :
Text Solution
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Two flask initally at 27 0 and 0.5 atm, have same volume and 0.7 mole thus each flask has 0.35 mole
Let n mole of gas are diffuse from II to I on heating the flask at 127 0 C
Mole in I flask = 0.35 + n,
Mole in II flask = 0.35 – n
If new pressure of flask is P then
for I flask P × V = (0.35 + n) × R × 300 ;
for II flask P × V = (0.35 – n) × R × 400
n = 0.5
mole in I flask = 0.40 mole in II flask = 0.30
0.5 × 2V = 0.7 × 0.0821 × 300 (initially)
V = 17.24 Lt.
P × 17.24 = 0.30 × 0.0821 × 400 (finally)
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