Asked by erica
From the reaction below, calculate the free energy of formation for CH4(g) at 25°C, if ΔGfo(C8H8(g)) is 214.417 kJ/mol.
8CH4(g) ↔ C8H8(g) + 12H2(g) ΔGo = 620.735 kJ/mol
I don't understand what equation to use. I thought it was dGfo-dGo but that doesn't give the right answer.
8CH4(g) ↔ C8H8(g) + 12H2(g) ΔGo = 620.735 kJ/mol
I don't understand what equation to use. I thought it was dGfo-dGo but that doesn't give the right answer.
Answers
Answered by
DrBob222
I believe you forgot the coefficients (e.g. 8).
8CH4 ==> C8H8+ 12H2
dGfrxn = (n*dGfC8H8 + n*dGfH2)-(n*dGfCH4)
620.735 = [(1*214.417) + (12*0)] - (8*dGfCH4)
620.735 = 214.417 + 0 - 8x
Solve for x.
8CH4 ==> C8H8+ 12H2
dGfrxn = (n*dGfC8H8 + n*dGfH2)-(n*dGfCH4)
620.735 = [(1*214.417) + (12*0)] - (8*dGfCH4)
620.735 = 214.417 + 0 - 8x
Solve for x.
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