The oxidation of solid glucose (C6H12O6) to carbon dioxide gas(CO2) and liquid w
ID: 678673 • Letter: T
Question
The oxidation of solid glucose (C6H12O6) to carbon dioxide gas(CO2) and liquid water(H2O) at 298.15 K and 1 bar pressure is accompanied by an enthalpychange of -2808 kJ/mol.
C6H12O6(s) + 6O2 (g) -> 6CO2 (g) + 6H2O(l)
a) What is the standard Gibbs energy change of this reaction at298.15K?
b) What is the change in the TOTAL entropy of the system +surroundings after this
reaction takes place?
c) If the pressure is increased slightly, does this make thereaction more or less
spontaneous? Why? The oxidation of solid glucose (C6H12O6) to carbon dioxide gas(CO2) and liquid water
(H2O) at 298.15 K and 1 bar pressure is accompanied by an enthalpychange of -2808 kJ/mol.
C6H12O6(s) + 6O2 (g) -> 6CO2 (g) + 6H2O(l)
a) What is the standard Gibbs energy change of this reaction at298.15K?
b) What is the change in the TOTAL entropy of the system +surroundings after this
reaction takes place?
c) If the pressure is increased slightly, does this make thereaction more or less
spontaneous? Why?
Explanation / Answer
C6H12O6(s) + 6O2(g).......>6CO2 (g) + 6H2O(l) a. G0rxn ={6G0(CO2(g))+6G0(H2O(l))}-{1G0(C6H12O6(s))+6G0(6O2(g))} = {6(-394.4)+6(-237.13)kJ}-{1(-910.4)+6(230.1)}kJ =-3789.18kJ -470.2kJ = -4259.38kJ b. H0rxn = {6H0(CO2(g))+6H0(H2O(l))}-{1H0(C6H12O6(s))+6H0(6O2(g))} = {6(-393.5)+6(-285.83)}-{1(-1273.02)+6(0)}kJ H0rxn =-2802.96kJ S0surr = -H0sys / T = -(-2802.96kJ) / 298.15K = 9.4011kJ/K S0surr = 9401.1J/K S0rxn = {6Sf0(CO2(g))+6Sf0((H2O(l))} -{1Sf0((C6H12O6(s))+6Sf0(O2(g))} ={6(213.6)+6(69.91)}J/K-{1(212.1)+6(205.0)}J/K S0rxn =258.96J/K S0rxn = S0sys =258.96J/K S0univ =S0sys + S0surr = 258.96J/K + 9401.1J/K =9660.06J/KRelated Questions
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