The chemical reaction that causes chromium to corrode in air is given by 4Cr+3O2→2Cr2O3 in which at 298 K ΔH∘rxn = −2256 kJ ΔS∘rxn = −549.1 J/K Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K.

The standard gibbs free energy for this reaction is -2092.4 kJ

Explanation:

Step 1: Data given

Temperature = 298 K

ΔH° rxn = −2256 kJ

ΔS° rxn = −549.1 J/K

Step 2: The balanced equation

4Cr + 3O2 → 2Cr2O3

Step 3:

The formula for the gibbs free energy is:

ΔG° = ΔH° - T * ΔS°

⇒with ΔG° = the gibbs free energy for this reaction = TO BE DETERMINED

⇒with ΔH° = the standard enthalpy of the reaction  = −2256 kJ

⇒with T = the temperature of the reaction in Kelvin = 298 K

⇒with ΔS°  = standard entropy of the reaction = −549.1 J/K

ΔG° = -2256 kJ - 298 K* (-0.5491 kJ/K)

ΔG° = -2256 kJ + 163.6318 kJ

ΔG° = -2092.4 kJ

The standard gibbs free energy for this reaction is -2092.4 kJ

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

la respuesta es si te gusta hacer lo que siempre haces cuando nunca ves a alguien en el espejo porque sabes que no siempre están ahí.