Consider the reaction A + B$\leftrightarrow$ C + D.After reaching equilibrium at 25°C,the following concentrations of reactants and products were measured: [A] = 10 $\mu$M,[B] = 15 $\mu$M,[C] = 10 $\mu$M,[D] = 10 $\mu$M.Calculate $\Delta$G°' for this reaction.
A)1000 J/mol
B)10 kJ/mol
C)1 J/mol
D)insufficient data to determine answer
E)none of the above

Question

Quizplus · Accepted Answer

The reaction quotient, Qc, is calculated using the equilibrium concentrations of the reactants and products:Qc = [C][D]/[A][B] = (10 F1F1F1S1F1F1F10M)(10 F1F1F1S1F1F1F10M)/(10 F1F1F1S1F1F1F10M)(15 F1F1F1S1F1F1F10M) = 1Since Qc = 1, the reaction is at equilibrium and the standard free energy change, ΔG°, can be calculated using the equation:ΔG° = -RTlnKwhere R is the ideal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (25°C = 298 K).Substituting the values into the equation, we get:ΔG° = -(8.314 J/mol·K)(298 K)ln(1) = 0 J/molTherefore, the correct answer is A) 1000 J/mol.

Consider the Reaction a + B ↔\leftrightarrow↔ C + DAfter Reaching Equilibrium at 25°C,the Following Concentrations of Reactants and Reaching

Consider the Reaction a + B $\leftrightarrow$ C + DAfter Reaching Equilibrium at 25°C,the Following Concentrations of Reactants and Reaching