Calculate Delta H and Delta S (1 of 3)

Question

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.

C6H12O6 (s) 6 O2 (g) ====> 6 CO2 (g) 6 H2O (l)

Answer 1

C6H12O6 (s)

dHf = -1273.02 kJ

S = 212.1J

6 O2 (g

dHf = 0

S = (6) (205 J) = 1230J

6 CO2 (g

dHf = (6) (- 393.5) = -2361kJ

S = (6) (213.6J) = 1281.6J

6 H2O (l)

dHf = (6)(-285.83)= -1714.98 kJ

S = (6) (69.91) = 419.46J

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C6H12O6 (s)&   6 O2 (g) ====> 6 CO2 (g) &   6 H2O (l)

dH = prod - reactants

dH = ( -1714.98  & -2361 ) - (0  &    -1273.02 kJ)

Your answer: dH = - 2802.96 kJ

dS = prod - reactants

dS = (419.46 & 1281.6J) - (1230  & 212.1J )

your answer is: 258.96 J

with needing a dG = - to be spontaneous,

& dG = dH -TdS

your answer is: product favored always product favored,

& that is because the dH prodides the desired "-",  and at any temp,

-TdS will always provide a "-"