Asked by Gabby
Methanol is an organic solvent and is also used as fuel in some automobile engines. From the following data, calculate the standard enthalpy of formation of methanol.
2CH3OH + 3O2 --> 2CO2 + 4H2O, (delta H = -1452.8 kJ/mol
2CH3OH + 3O2 --> 2CO2 + 4H2O, (delta H = -1452.8 kJ/mol
Answers
Answered by
ash
(2*-393.5+4*-242)-(2*-293+0)
Delta H+ -1169 kJ/mol
Delta H+ -1169 kJ/mol
Answered by
DrBob222
I don't agree with the answer provided by ash.
dHxn = (n*dHf products) - 2x = -1452.
Solve for x for dHf CH3OH.
dHxn = (n*dHf products) - 2x = -1452.
Solve for x for dHf CH3OH.
Answered by
Zander
just had this question on my webassign-
products
h2o is liquid: dH= -286 kJ (x4)
CO2 (g): dH= -393.509 kJ (x2)
reactants:
CH3OH (l): dH= 2dH (unknown)
O2 (g): dH= 0 (x3) (0 bc its elemental)
dH(rxn) = dH(prod) - dH(react)
-1452.8= -1931.018 - 2dH(CH3OH)
-2dH(CH3OH) = 478.218
dH(CH3OH) = -239.109
products
h2o is liquid: dH= -286 kJ (x4)
CO2 (g): dH= -393.509 kJ (x2)
reactants:
CH3OH (l): dH= 2dH (unknown)
O2 (g): dH= 0 (x3) (0 bc its elemental)
dH(rxn) = dH(prod) - dH(react)
-1452.8= -1931.018 - 2dH(CH3OH)
-2dH(CH3OH) = 478.218
dH(CH3OH) = -239.109