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A 21.2-L sample of nitrogen at 3.65 atm and 22 degree C is simultaneously expanded to 62.6 L and heated to 34 degree C. What is the new pressure of the gas? 1.91 atm 1.29 atm 235 atm 349 atm 1.19 atm
Expert Answer
We know that PV = nRT
Where
T = Temperature ;P = pressure ; n = No . of moles ;R = gas constant ; V= Volume of the gas
As the gas remains the same , n will constant
So PV / T = constant
Thereby PV/T = P’V’/T’
Where
P = initial pressure = 3.65 atm
V = initial volume = 21.2 L
T = initial temperature = 22.0 oC = 22.0+273 = 295 K
P’= final pressure = ?
V’ = final volume = 62.6 L
T’ = final temperature = 34oC = 34+273 = 307 K
Plug the values we get P’ = (PVT’)/(TV’) = 1.29 atm
