In: Chemistry
A bottle at 325 K contains an ideal gas at a pressure of 1.613×105 Pa . The rubber stopper closing the bottle is removed. The gas expands adiabatically against \(P_{external} \ = \\) 1.168×105 Pa , and some gas is expelled from the bottle in the process. When P = Pexternal , the stopper is quickly replaced. The gas remaining in the bottle slowly warms up to 325 K What is the final pressure in the bottle for a monatomic gas, for which CV,m = 3R/2?
Given,
The initial temperature T = 325 K
Pressure P = 1.613*105 Pa
After the gas expands adiabatically,
P' = 1.168 * 105 Pa
Temperature = T'
For a adiabatic process,
P1- * T= constant
P1- * T= P'1- * T'
T / T' = (P' / P)(1-) / .........(1)
For the gas inside the bottle after stopper is quickly replaced,
Pi = P'
Ti = T'
Tf = T
Here, volume is constant,
Hence, P' / T' = Pf / T
Pf = P' * (T / T')
Put the value of T / T' from eq(1)
Pf = P' * (P' / P)(1-) /
Pf = P'1/* P-1 /
For monatomic gas CV,m = 3R/2, = 5/3),
Pf = (1.168*105 )3/5 * (1.613*105)(5/3 - 1) / 5/3
Pf = (1.0976*103) * ((1.613*105)(2/5)
Pf = (1.0976*103) *(1.2107*102)
Pf = 1.3288*105 Pa