5.10 g of nitrogen gas at 18.0 degree C and an initial pressure of 2.90 atm unde

Question

5.10 g of nitrogen gas at 18.0 degree C and an initial pressure of 2.90 atm undergo an isobaric expansion until the volume has tripled. How much heat energy is transferred to the gas to cause this expansion? Express your answer with the appropriate units. The gas pressure is then decreased at constant volume until the original temperature is reached. What is the gas pressure after the decrease? Express your answer with the appropriate units. What amount of heat energy is transferred from the gas as its pressure decreases? Express your answer with the appropriate units.

Explanation / Answer

heat required=nCp*change in temperture

PV=nRT

V=nRT/P=3*10^(-3) m^3

for isobaric

P*change in volume=nR*change in temperature

change in temperature=873 -291=582 K

heat required=6169.4 J

B

final pressure=2.9 atm

final temp=873 K

now volume is constant so

P1/T1=P2/T2

we got

P2=P1*T2/T1=0.967 atm

part C

heat =nCp*change in temp=6169.4 J

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