The ΔH of the reaction below is -575.13 kJ. Is this reaction spontaneous?
2ZnS + 3O2 + C → 2SO2 + 2Zn + CO2
A. It is not because the ΔH of the reaction is negative.
B. It is because the ΔH of the reaction is negative.
C. It depends on the temperature because the ΔH of the reaction is negative and the ΔS is negative.
D. It depends on the temperature because the ΔH of the reaction is negative and the ΔS is positive.
To determine if a reaction is spontaneous, we need to consider both the enthalpy change (ΔH) and the entropy change (ΔS) of the reaction.
In this case, we are given the enthalpy change (ΔH) of the reaction, which is -575.13 kJ. A negative ΔH indicates an exothermic reaction, which means that the reaction releases heat and the products have lower energy than the reactants.
However, the information provided does not include the entropy change (ΔS) of the reaction. The entropy change reflects the disorder or randomness of the system. Since we don't have the value of ΔS, we cannot directly determine if the reaction is spontaneous.
Thus, the correct answer is either C. It depends on the temperature because the ΔH of the reaction is negative and the ΔS is negative or D. It depends on the temperature because the ΔH of the reaction is negative and the ΔS is positive. The spontaneity of a reaction depends on both the enthalpy and entropy changes, as well as the temperature.