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for the oxidation of iron to form iron(iii)oxide
4Fe(s)+3O2(g)=2Fe2O3(s) deltaS^o=-549.73J×K^-1 at 298K
the enthalpy of formation of Fe2O3(s) is -824.2 kj×mol^-1. what is the standard change in gibbs free energy for this reaction at 298K? Delta G^o=delta H^o-T delta S^o

Sagot :

minmayoo

Answer:

only god knows the answer

The Gibbs free energy is given by the change in enthalpy, temperature, and change in entropy. The standard change in Gibbs free energy for oxidation of iron is –1484.6 kJ.

What is Gibbs free energy?

Gibbs free energy is the energy present in a thermodynamic system that is used by the reactant to form a product. It is given as,

Δ G° = Δ H° -T ΔS°

The oxidation reaction of iron is given as,

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

Given,

ΔS° = –549.73 J∙K⁻¹

T = 298 K

Δ H° = –824.2 kJ∙mol⁻¹

Substituting values above the Gibbs free energy is calculated as:

Δ G° = Δ H° -T ΔS°

= –824.2 kJ∙mol⁻¹ -  298 K ( –549.73 J∙K⁻¹)

= -1484580.46 J

The units of joules are converted into kilojoules and the standard change in Gibbs free energy will be –1484.6 kJ.

Therefore, –1484.6 kJ is the Gibbs free energy.

Learn more about Gibbs free energy here:

https://brainly.com/question/13318988

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