One mole of a perfect gas expands isothermally to ten times its original volume the change in entropy at 298 k will be
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Answer:
2.303R.
Explanation:
From the question we have that it will be isothermal expansion, hence there will not be any change in temperature and internal energy. So, TΔS will be dU+pdV. Since dU =0 so we will have ΔS=PdV/T
Since, we know that the PV=nRT, So, the ΔS will be nRdV/V.
So, the change in the entropy will be equal to.
S2 - S1 = nRln(V2/V1)
On substituting the values of n, R and volume we will have that v2/v1=10 and the number of moles is 1.
So, ΔS=2.303*1*R*log(v2/v1).
ΔS=2.303*R*log10 which on solving will be equal to ΔS=2.303R.
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