Question

Calculate the Gibbs energy, entropy, and enthalpy of mixing when 1.00mol C6H14 (hexane) is mixed with 1.00mol C7H16 (heptane) at 298K. Treat the solution as ideal.

Answer 1

With Hexane of 1.00 ml and 1.00 ml of hectane at 298, the calculated

• Gibbs energy = 3.43
• Entropy = -3.43
• Enthalpy = 0

How to solve for the Gibbs energy

C6H14 = C6H14/C6H14+C7H16

1mol/1mol+1mol = 1/2 = 0.5 mol

1+1 x 8.3145J x 298 x 0.5ln0.5 + 0.5ln0.5

= 4955.442 0.6932

= 3435J

convert to KJ

G mix = 3.43

The Gibbs energy is therefore  3.43KJ/mol

The entropy of the solution

-(1+1 x 8.3145J x 298 x 0.5ln0.5 + 0.5ln0.5)

S mix = -3.43 KJ/mol

3.43/298 = 11.5

The enthalpy of the solution

3.43-3.43 KJ/mol

H mix = 0

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