#19 a) b) c) d) e) 2.50 moles of an ideal gas, initially at a volume of 4.00 m^3
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Question
#19
a)
b)
c)
d)
e)
2.50 moles of an ideal gas, initially at a volume of 4.00 m^3 and a pressure of 2.00 atm, are subjected to the following four processes, in order: i. Its volume is decreased isobarically to 1.00 m^3. ii. Its pressure is increased isovolumetric to 6.00 atm. iii. Its volume is increased isobarically to 4.00 m^3. iv. Its pressure is decreased isovolumetric to 2.00 atm. For the overall process: a. Draw a PV diagram. b. Find the lowest temperature of the gas during the process. c. Find the highest temperature of the gas during the process. d. Find the total work done by the gas on its environment. e. Find the total amount of heat transferred to the environment.Explanation / Answer
Here work done=Area under PV graph
=length x breadth
=3m^3x5atm
Finding temperature use below formula
PV=NRT
Ti=PV/NR
= 2x1.01*10^5x4/2.50* 8.314
Tf=PV/NR
=1X6X1.01X10^5/2.50*8.314
Q=NRT
=2.50*8.314*(Tf_Ti)
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