REMARKS The exact answer, obtained with calculus, Is -8.43 x 104 J, so our resul
ID: 2036967 • Letter: R
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REMARKS The exact answer, obtained with calculus, Is -8.43 x 104 J, so our result is a very good estimate. The answer is negative because the gas is expanding, doing positive work on the environment, thereby reducing its own internal energy. QUESTION For an adiabatic expansion between two given volumes and an initial pressure, which gas does more work, a monatomic gas or a diatomic gas? Why? O A diatomic gas does more work because of the greater mass of the molecules colliding with the walls of the container. OA diatomic gas does more work because 1 mole of diatomic gas contains more molecules. O Both do the same work, because the pressure is the same at each volume, according to the ideal gas law O A diatomic gas does more work because its temperature, and therefore its pressure, is lowered less by the work it does. O A monatomic gas does more work because its temperature, and therefore pressure, is lowered less by the work it does. EXERCISE HINTS: GETTING STARTED I I'M STUCK! Repeat the preceding calculations for an ideal diatomic gas expanding adiabatically from an initial volume of o.500 m3 to a final volume of 1.25 m3, starting at a pressure of 1.01 x 105 Pa, (You must sketch the curve td find the work.) PaExplanation / Answer
4th Option is correct as the diatomic gases have more degree of freedom enabling to loosen the heat quickly.
Assume y= Heat capacity ratio
PV^y=constant
P2V2^y=P1V1^y
P2=0.22*10^5 Pa
W=(P2V2-P1V1)/(1-y)=0.345 J
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