Gibbs free energy (g) is a measure of the spontaneity of a chemical reaction. it is the chemical potential for a reaction, and is minimized at equilibrium. it is defined as g=h−ts where h is enthalpy, t is temperature, and s is entropy. the chemical reaction that causes magnesium to corrode in air is given by 2mg+o2→2mgo in which at 298 k δh∘rxn = −1204 kj δs∘rxn = −217.1 j/k part a what is the standard gibbs free energy for this reaction? assume the commonly used standard reference temperature of 298 k. express your answer as an integer and include the appropriate units. view available hint(s) δg∘rxnδ g r x n ∘ = nothing

ΔG° = -1123 kJ

Explanation:

Let's consider the following equation.

2 Mg + O₂ → 2 MgO

The standard Gibbs free energy (ΔG°) can be calculated with the following expression:

ΔG° = ΔH° - T.ΔS°

where,

ΔH° is the standard enthalpy of the reaction

T is the absolute temperature

ΔS° is the standard entropy of the reaction

For this reaction,

ΔG° = -1204 kJ - 298 K × (-271.1) × 10⁻³ kJ/K = -1123 kJ

By convention, ΔG° < 0 means that the reaction is spontaneous.

hloride, what is the mass of calcium in

explanation:

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons