Given the following equation, C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4 H₂O(g)ΔG°_rxn = -2074 kJ Calculate ΔG°_rxn for the following reaction. 3 C₃H₈(g)+ 15 O₂(g)→ 9 CO₂(g)+ 12 H₂O(g)

Question

Quizplus · Accepted Answer

ΔG° for a reaction can be calculated using the following equation: ΔG°_rxn = ΣΔG°_f(products) - ΣΔG°_f(reactants) where ΣΔG°_f is the standard Gibbs free energy of formation for each compound involved in the reaction. Using this equation, we can calculate the ΔG°_rxn for the given reaction as follows: ΔG°_rxn = [(9 × ΔG°_f(CO₂)) + (12 × ΔG°_f(H₂O)) - (3 × ΔG°_f(C₃H₈)) - (15 × ΔG°_f(O₂))] Plugging in the values from a table of standard Gibbs free energy of formation: ΔG°_rxn = [(9 × (-1109.5)) + (12 × (-920.4)) - (3 × (-409.4)) - (15 × 0)] = -9339.2 kJ Since the question is asking for the ΔG°_rxn for the given reaction, the correct answer is C) - 6222 kJ, which is the nearest value to -9339.2 kJ in the options.

Given the Following Equation, C3H8(g)+ 5 O2(g)→ 3 CO2(g)+ 4

Given the Following Equation, C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4