Which of the following is the equilibrium constant for the reaction below at 25 °C? (R = 8.314 J/K ⋅mol) MgCO3(s) MgO(s) + CO2(g); ΔfG° [MgCO3(s)] = -1028.2 kJ/mol, ΔfG [MgO(s)] = -568.8 kJ/mol, and ΔfG° [CO2(g)] = -394.4 kJ/mol. A) 4.0 × 10^-12 B) 0.97 C) 1.0 D) 1.0 × 10⁴ E) 2.5 × 10¹¹

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Quizplus · Accepted Answer

The equilibrium constant (K) is given by the equation:K = exp(-ΔG°/RT)where ΔG° is the standard free energy change, R is the gas constant, and T is the temperature in Kelvin.Plugging in the given values, we get:K = exp(-(-1028.2 kJ/mol - (-568.8 kJ/mol - (-394.4 kJ/mol))/(8.314 J/K ⋅mol)(298 K))= 4.0 × 10^-12

Which of the Following Is the Equilibrium Constant for the Reaction