What is the standard Gibbs free energy for this reaction? Assume the commonly us

Question

What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. The chemical reaction that causes magnesium to corrode in air is given by

2Mg+O2?2MgO

in which at 298 K

?H?rxn = ?1204 kJ ?S?rxn = ?217.1 J/K ± Gibbs Free Energy: Temperature Dependence The chemical reaction that causes magnesium to corrode in air is given by Mg + O22Mgo Gibbs free energy (G) is a measure of the spontaneity ofa chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as in which at 298 K Alan=-1204 kJ G=H-TS 217.1 J/K where H is enthalpy, T is temperature, and S is entropy. 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. HA 9 kJ Subit Hints My Answers Give Up Review Part Incorrect; Try Again; 2 attempts remaining You may have forgotten to convert the temperature to kelvins. Submit You may need to review Conv

Explanation / Answer

Delta G = Delta H - T Delta S

Delta H = -1204 KJ / mole

Delta S = -217.1 J / mole = -0.2171 KJ / mole

Delta G = -1204 - 298 X (-0.2171) = -1204 + 64.69 = -1139.31 KJ

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