The value of ΔG° for the following reaction is -5490. kJ. ?
calculate the standard free energy of formation for C4H10(g).
2 C4H10(g) + 13 O2(g)====>8 CO2(g) + 10 H2O(l)
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calculate the standard free energy of formation for C4H10(g).
2 C4H10(g) + 13 O2(g)====>8 CO2(g) + 10 H2O(l)
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2 C4H10(g) + 13 O2(g)====>8 CO2(g) + 10 H2O(l)
dG reaction = dGf's products - reactants
dG = [(8mol CO2@ -394.4kJ/mol) & (10mol H2O @ -237.13kJ/mol)] -
[(dGf for 2mol C4H10) & (zero for oxygen)]
-5490 = -3155.2 & -2371.3 - (dGf for 2mol C4H10)
5490 = 3155.2 & 2371.3 + (dGf for 2mol C4H10)
(dGf for 2mol C4H10) = 5490 - 3155.2 - 2371.3
(dGf for 2mol C4H10) = -36.5
(dGf C4H10) = -18.25 kJ/mol
(you will have to compare my text's dGf with yours, they rarely agree)
my textbook has dGf pf C4H10 = - 15.71kJ/mol)