Gibbs Free Energy Calculation Unit Error
A student calculates the standard Gibbs free energy change, ∆G°, for a reaction at 298 K using the equation ∆G° = ∆H° - T∆S°. The student uses ∆H° = -150 kJ/mol and ∆S° = 250 J/mol·K, but neglects to convert the units of ∆S° to be consistent with the units of ∆H°. What is the effect of this error on the calculated ∆G° and the determination of the reaction’s spontaneity?
The calculation of ∆G° is unaffected by the unit of ∆S°, and the assessment of spontaneity remains accurate.
The calculation of ∆G° is incorrect due to the failure to convert ∆S° to kJ/mol·K, likely leading to an incorrect assessment of spontaneity.
The omission of temperature in the calculation of ∆G° is the primary error, affecting the spontaneity assessment.
Converting ∆S° from J/mol·K to kJ/mol·K is unnecessary as ∆H° and ∆S° units cancel out in the equation.
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