Question

One mole of a perfect gas expands isothermally to ten times its original volume the change in entropy at 298 k will be​

Answer 1

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.