Given the following information determine the reaction Gibbs energy for the formation of silicon dioxide at 298 K
Si(s)+O2(g) →SiO2(s)
ΔfH°(Si(s))=0 kJ mol-1, S°(Si(s))=18.8 J mol-1 K-1
ΔfH°(O2(g))=0 kJ mol-1, S°(O2(g))=205.0 J mol-1 K-1
ΔfH°(SiO2(s))=-910.7 kJ mol-1, S°(SiO2(s))=41.8 J mol-1 K-1
Answer to TWO decimals places in kJ mol-1
1 answer
dHo rxn = (n*dHo products) - (n*dHo reactants)