Gaseous StateHard
Question
Two flasks of equal volume are connected by a narrow tube (of negligible volume) all at 27oC and contain 0.70 moles 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 number of moles of H2 in flask 1 and flask 2 are :
Options
A.Moles in flask 1 = 0.4, Moles in flask 2 = 0.3
B.Moles in flask 1 = 0.2, Moles in flask 2 = 0.3
C.Moles in flask 1 = 0.3, Moles in flask 2 = 0.2
D.Moles in flask 1 = 0.4, Moles in flask 2 = 0.2
Solution
Let vol. of each flask is ′V′ L, Initially
0.5 × 2V = 0.7 × 0.0821 × 300
V = 17.24 L
Let T is final temperature of flask when pressure in each flask becomes equal, it happens. when
nTotal = n1 + n2
⇒ 
T =
= 342.85 K
P × 2 × 17.24 = n1 × 0.0821 × 400 ⇒ n1 = 0.3
0.5714 × 17.24 = n2 × 0.0821 × 300 ⇒ n2 = 0.4
0.5 × 2V = 0.7 × 0.0821 × 300
V = 17.24 L
Let T is final temperature of flask when pressure in each flask becomes equal, it happens. when
nTotal = n1 + n2
⇒ T =
= 342.85 KP × 2 × 17.24 = n1 × 0.0821 × 400 ⇒ n1 = 0.3
0.5714 × 17.24 = n2 × 0.0821 × 300 ⇒ n2 = 0.4
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