Hello Chemists,
I have been given this question in an assignment worth 10 marks. I am a bit perplexed because I think it's a rather simply question, however it's worth 10 marks!
Would someone be so kind to review my question and tell me if I am on the correct path?
calculate the ΔGo(C8H18) at 25oC of octane.
2C8H18 (l) + 25O2 (g) ----------> 16 CO2 (g) + 18 H20 (l)
ΔGo(C8H18) = ΔHo - TΔSo
ΔGo(C8H18) = (-208.4 kJ/mol) – (298K) (0.4637 kJ/K.mol)
ΔGo(C8H18) = (-208.4 kJ/mol) – (138.2 kJ/mol)
ΔGo(C8H18) = - 346.6 kJ/mol
However because there are 2 moles of C8H18 in the original reaction the 2ΔGo(C8H18) = -693.2 kJ/mol
ΔGorxn= [16(-394.4 kJ/mol) + 18(-237.2 kJ/mol)] – [2(-346.6 kJ/mol) + 25(0 kJ/mol)] =
ΔGorxn= [-6310.4 kJ/mol + -4269.6 kJ/mol] – [-693.2 kJ/mol] =
ΔGorxn= [-10580 kJ/mol)] – [-693.2 kJ/mol)] = -9886.8 kJ/mol
Therefore because ΔGorxn < 0 this reaction is sponateous.
Thank you so much for your time chemists,
Have a great day!