In: Chemistry
If 20.00 mol of helium gas is at 17.0 ∘C and a gauge pressure of 0.320 atm .
Calculate the temperature in celcius if the gas is compressed to precisely half the volume at a gauge pressure of 1.00 atm. Original volume is 0.3608m3
Moles of Helium gas = 20.00 mol
Initial conditions of Helium gas:
Given that helium gas is at 17 oC and a gauge pressure of 0.320 atm , original volume is 0.3608 m3
Pressure P1 = 0.320 atm
Volume V1 = 0.3608 m3
Temperature T1 = 17 oC = 17 + 273 K = 290 K
Final conditions of Helium gas:
Given that Helium gas is compressed to precisely half the volume at a gauge pressure of 1.00 atm.
Pressure P2 = 1.00 atm
Volume V2 = V1 /2 = 0.1804 m3
Temperature T2 = ?
We know that
P1V1/T1 = P2V2/T2
T2 = (P2V2) (T1/P1V1)
= ( 1.00 atm x 0.1804 m3) ( 290K / 0.320 atm x 0.3608m3)
= 453.125 K
= 180.125 oC
T2 = 180.125 oC
Therefore, final temperature of the Helium gas = 180.125 oC