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Delta G (written triangle G) = Delta H -T Delta S
The change in enthalpy between products and reactants in a reaction
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
The change in enthalpy between products and reactants in a reaction
4Fe(s) + 3O2(g) --> 2Fe2O3(s)
The change in enthalpy between products and reactants in a reaction
Delta G (written triangle G) = Delta H -T Delta S
Delta G (written triangle G) = Delta H -T Delta S
Delta G (written triangle G) = Delta H -T Delta S
The change in enthalpy between products and reactants in a reaction
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
Use the following equation: delta G = delta H - T*deltaS. A reaction is spontaneous if delta G is negative. A reaction will always be spontaneous (under any temperature) only if the change in enthalpy (delta H) is negative and the change in entropy (delta S) is positive. If this is not the case, the reaction will only be spontaneous (negative delta G) for a range of temperatures (or could be always non-spontaneous)
The change in enthalpy between products and reactants in a reaction
G is always positive when enthalpy increases and entropy decreases.
Unfortunately, you did not specify what final chemical equation you wanted given these formulas. From the data though I assumed the following: Fe2O3(s) + 3CO(g) à 2Fe(s) + 3CO2 H1 3Fe2O3(s) + CO(g) à 2Fe3O4(s) + CO2(g) H2 Fe3O4(s) + CO(g) à 3FeO(s) + CO2(g) H3 3(Fe2O3(s) + 3CO(g) à 2Fe(s) + 3CO2) 3(H1) 2Fe3O4(s) + CO2(g) à3Fe2O3(s) + CO(g) -H2 2(3FeO(s) + CO2(g) à Fe3O4(s) + CO(g)) 2(-H3) 3Fe2O3(s) + 9 (6)CO(g) à 6Fe(s) + 9(6)CO2 3(H1) 2Fe3O4(s) + CO2(g) à3Fe2O3(s) + CO(g) -H2 6FeO(s) + 2CO2(g) à 2Fe3O4(s) + 2CO(g) 2(-H3) 6FeO(s) + 6CO(g) à 6Fe(s) + 6CO2 3H1 + -H2 + -2H3 FeO(s) + CO(g) à Fe(s) + CO2 [(3H1 + -H2 + -2H3) / 6] FeO(s) + CO(g) à Fe(s) + CO2 -11KJ/mol
+delta H, -delta S, +delta G