What temperature (in °C) did an ideal gas shift to if it was initially at -10.0 °C at 4.62 atm and 35.0 L and the pressure was changed to 8.71 atm and the volume changed to 15.0 L?
Hi we can use ideal gas equation for this purpose here
PV = nRT, n & R are constant
P1V1 / P2V2 = T1 / T2
P1 = initial pressure = 4.62 atm; V1 = initial volume = 35 L; T1 = -10 oC = -10 + 273 = 263 K;
P2 = final pressure = 8.71 atm; V2 = final volume = 15L; T2 = final temp =
T2 = (P2V2 / P1V1) x T1 = [(8.71 atm x 15 L) / (4.62 atm x 35 L)] x 263 K
T1 = 212.498144712 = 212.5 K = 212 - 273 = -60.5 oC
Answer: -60.5 oC (negative sign present)
Hope this helped you!
Thank You So Much! Please Rate this answer as you wish.("Thumbs Up")
Get Answers For Free
Most questions answered within 1 hours.