Question:

Calculate Delta H and Delta S (2 of 3)

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Calculate delta H and delta S for the following reaction and predict whether the reaction is either: always product favored, product favored at only at low temperatures, product favored only at high temperatures, or never product favored.

FeO3 (s) 2 Al (s) ===> 2 Fe (s) Al2O3 (s)

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  1. Fe2O3 (s)

    dHf = - 822.16 kJ

    S = 89.96J



    2 Al (s)

    dHf = 0

    S = (2) (28.32 J) = 56.64J

    2 Fe (s)

    dHf = 0

    S = (2) (27.15J) = 54.30J

    Al2O3 (s)

    dHf = - 1669.8 kJ

    S = 51J

    ===========================

    Fe2O3 (s) &  2 Al (s) ===> 2 Fe (s) & Al2O3 (s)

    dH = prod - reactants

    dH = (- 1669.9) - ( - 822.16 kJ)

    Your answer: dH = - 847.9 kJ

    dS = prod - reactants

    dS = (51 & 54.3) - (56.64  & 89.96J)

    your answer is: - 41.3 J

    with needing a dG = - to be spontaneous,

    & dG = dH -TdS

    your answer is: product favored at only at low temperatures,

    & that is because the dH prodides the desired "-",  but @ high temps,

    -TdS will provide a "+" that will eventually over power the "-" of the dH

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