Question

The absolute molar entropies of O2 and N2 are 205 J K-1 mol -1 and 192 J K-1 mol-1, respectively, at 25°C. What is the entropy of a mixture of 2.4 moles of 02 and 9.2 moles of N2 at the same temperature and pressure?

Answer 1

The entropy of a mixture is 96.44J K-1 mol -1

• The absolute molar entropies of O2= 205 J K-1 mol -1

• The absolute molar entropies of N2=192 J K-1 mol -1
• Moles of O2 present(m)=2.4
• Moles of N2 present(n)=9.2

The formula for calculating the entropy of a mixture-

Δ$S_{mix} =$$-nR(X_{O2} ln_{XO2} +X_{N2} lnX_{N2})$

X=mole fraction

total no. of moles(t)=m + n

                             =2.4+9.2

                             =11.6 moles

now substituting the values-

entropy of mix=-11.6R(2.4/11.6 + 9.2/11.6)

                       =11.6R

( R=8.314 )        =11.6×8.314

                          =96.44J K-1 mol -1

hence, The entropy of a mixture is 96.44J K-1 mol -1

learn more about entropy here:

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