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Question
Figure shows two rigid vessels A and B, each of volume 200 cm3, containing an ideal gas (Cv = 12.5 J K−1 mol−1). The vessels are connected to a manometer tube containing mercury. The pressure in both the vessels is 75 cm of mercury and the temperature is 300 K. (a) Find the number of moles of the gas in each vessel. (b) 5.0 J of heat is supplied to the gas in vessel A and 10 J to the gas in vessel B. Assuming there's no appreciable transfer of heat from A to B, calculate the difference in the heights of mercury in the two sides of the manometer. Gas constant, R = 8.3 J K−1 mol−1.
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Solution
Given:
Volume of gas in each vessel, V = 200 cm3
Specific heat at constant volume of the gas, Cv = 12.5 J/mol-K
Initial temperature of the gas, T = 300 K
Initial pressure of the gas, P = 75 cm of Hg
(a) Using the ideal gas equation, number of moles of gases in each vessel,
75 cm of Hg = 99991.5 N/m2
`"n" = ("P""V")/("R""T")`
`= (99991.5 xx 200 xx 10^-6)/(8.3 xx 300)`
= 8031.4 xx 10-6
=0.008
(b) Heat is supplied to the gas, but dV is zero as the container has rigid walls.
So, dW = P Δ V = 0
From first law of thermodynamics,
dQ = dU
⇒ 5 = nCvdT
⇒ 5 = 0.008 × 12.5 × dT
⇒ dT = 50 for A
`"P"/"T" = "P"_"A"/"T"_"A" ` because volume is kept constant.
Q = nCvdT
`"T" = "Q"/("n""C"_"v")`
`75/300 =( "P"_"A" xx 0.008 xx 12.5)/5`
`"P"_"A" = (75 xx 5)/(300 xx 0.008 xx 12.5)`
= 12.5 cm of Hg
Again ,` "P"/"T" = "P"_"B"/"T"_"B" [ For container B]`
`75/300 =( "P"_"B" xx 0.008 xx 12.5 )/10`
PB = 25 cm of Hg
The distance moved by the mercury,
PB − PA = 25 − 12.5 = 12.5 cm
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