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Two moles of an ideal gas undergo a reversible isothermal expansion from 1.97×10−2 m^3 to 4.82×10−2 m^3 at a temperature of 20.0 C.

What is the change in entropy of the gas?

WORKING:

Using [tex]\Delta[/tex]S = nRIn(V2/V1)

= 2(8.31*ln(4.82*10^-2/1.97*10^-2)

ANS = -138.20 J/K

Is this correct? I can only enter it once on my website and I want to make sure this is right first time :)

What is the change in entropy of the gas?

WORKING:

Using [tex]\Delta[/tex]S = nRIn(V2/V1)

= 2(8.31*ln(4.82*10^-2/1.97*10^-2)

ANS = -138.20 J/K

Is this correct? I can only enter it once on my website and I want to make sure this is right first time :)

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