ΔG˚=141.7 kJ for the following reaction. Calculate ΔG: T=10˚C, [SO ₃] = 25mM, [SO₂] = 50mM, & [O₂] = 75 mM. 
2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g)

• A. – 6,437 J
• B. 39,938 J
• C. -155,127 J
• D. 138,865 J

Answer: (D)

Verified step by step guidance

1. Understand the relationship between standard Gibbs free energy change (ΔG˚) and actual Gibbs free energy change (ΔG) using the equation: ΔG = ΔG˚ + RT ln(Q), where R is the universal gas constant, T is the temperature in Kelvin, and Q is the reaction quotient.
2. Convert the temperature from Celsius to Kelvin by adding 273.15 to the given temperature: T(K) = 10 + 273.15.
3. Calculate the reaction quotient (Q) using the concentrations of the reactants and products: Q = ([SO2]^2 * [O2]) / ([SO3]^2). Substitute the given concentrations into this expression.
4. Use the universal gas constant R = 8.314 J/(mol·K) and the calculated temperature in Kelvin to compute the term RT ln(Q).
5. Substitute ΔG˚, RT ln(Q), and the calculated Q into the equation ΔG = ΔG˚ + RT ln(Q) to find the actual Gibbs free energy change (ΔG).