With the pressure held constant at 250 kPa , 43 mol of a monatomic ideal gas exp

Question

With the pressure held constant at 250 kPa , 43 mol of a monatomic ideal gas expands from an initial volume of 0.85 m^3 to a final volume of 1.6 m^3.

a) How much work was done by the gas during the expansion?
W= J

b) What was the initial temperature of the gas?
Ti= K

c) What was the final temperature of the gas?
Tf= K

d) What was the change of the internal energy of the gas?
DeltaU= J

e) How much heat was added to the gas?
Q= J



Help on any or all would be so much appreciated! I know PV=nRT is where I need to start, but I don't know how to put this together!

Explanation / Answer

a) Work done=PV=250*103*(1.6-0.85)=187500J

b)Ti=PV/nR=250*103*0.85/(43*8.314)=594.4 K

c)Tf=PV/nR=250*103*1.6/(43*8.314)=1119 K

d) U=nCv*T=43*1.5*8.314*(1119-594.4)=281318J

e)Q=W+U=187500J+281318J=468818J

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