APFIVE A student is determining the spontaneity of a chemical reaction at 298 K and calculates the Gibbs free energy change (∆G°) using the equation ∆G° = ∆H° - T∆S°. If the student uses ∆H° = -150 kJ/mol, T = 298 K, and ∆S° = 250 J/mol·K without converting ∆S° to kJ/mol·K, what impact does this have on the calculation of ∆G° and the assessment of reaction spontaneity?
Converting ∆S° from J/mol·K to kJ/mol·K is unnecessary as ∆H° and ∆S° units cancel out in the equation.
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 calculation of ∆G° is unaffected by the unit of ∆S°, and the assessment of spontaneity remains accurate.
The omission of temperature in the calculation of ∆G° is the primary error, affecting the spontaneity assessment.
Question Leaderboard
Not enough data yet to show leaderboard.