Gaseous StateHard
Question
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 127oC, while the other remains at 27oC. The final pressure in each flask is :
Options
A.Final pressure = 0.5714 atm
B.Final pressure = 1.5714 atm
C.Final pressure = 0.5824 atm
D.None of these
Solution
Two flask initally at 27o 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 127oC
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) P = 0.57 atm.
Let n mole of gas are diffuse from II to I on heating the flask at 127oC
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) P = 0.57 atm.
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