Which statement is true about the formation of CaCO₃(s)from CaO(s)and CO₂(g)at 1.00 atm? CaO(s)+ CO₂(g)→ CaCO₃(s) ΔH° = -178.7 kJ and ΔS° = -150.4 J/K

Question

Quizplus · Accepted Answer

The spontaneity of a reaction is determined by the Gibbs free energy change, which is given by the equation ΔG° = ΔH° - TΔS°, where T is the temperature in Kelvin. For a reaction to be spontaneous, ΔG° must be negative. From the given values of ΔH° and ΔS°, we can calculate ΔG° at different temperatures using the above equation. At low temperatures, the negative value of ΔH° dominates over the positive value of TΔS°, and ΔG° is negative, indicating that the reaction is spontaneous. At high temperatures, the positive value of TΔS° dominates over the negative value of ΔH°, and ΔG° becomes positive, indicating that the reaction is not spontaneous. Therefore, the correct answer is C, the reaction is spontaneous at low temperatures.

Which Statement Is True About the Formation of CaCO3(s)from CaO(s)and

Which Statement Is True About the Formation of CaCO₃(s)from CaO(s)and