What temperature (in °C) did an ideal gas shift to if it was initially at -22.5 °C at 4.33 bar and 35.0 L and the pressure was changed to 8.71 bar and the volume changed to 15.0 L?

Answer 1

Given information:

T1 = initial temperature = -22.5ºC = 250.65K

P1 = initial pressure = 4.33 bar

V1 = initial volume = 35.0 L

P2 = final pressure = 8.71 bar

V2 = final volume = 15.0 L

Asked to find final temperature = T2

Use the combined gas law...

P1V1/T1 = P2V2/T2 and solve for T2...

T2 = P2V2T1 / P1V1

T2 = (8.71)(15.0)(251) / (4.33)(35.0)

T2 = 216K

Converting to ºC...

216 -273 = -56.6ºC

(Please be sure to double check the math)