Answer:
The reaction is spontaneous only at high temperatures and nonspontaneous at low temperatures. So the best answer would be spontaneous only at high temperature.
Step-by-step explanation:
The spontaneity of a reaction can be determined by comparing the changes in enthalpy (DH°) and entropy (DS°).
In this reaction, DH° is -125 kJ/mol, indicating an exothermic reaction where heat is released. The negative sign indicates that the reaction is favorable in terms of enthalpy.
DS° is +253 J/K · mol, indicating an increase in disorder or randomness. The positive value of DS° suggests that the products have greater entropy than the reactants.
To determine the spontaneity of the reaction, we need to consider both DH° and DS°.
If a reaction is spontaneous, it means that it will occur without any external influence. In this case, a spontaneous reaction would have a negative value for Gibbs free energy change (DG°). The equation for calculating DG° is:
DG° = DH° - TDS°
where T is the temperature in Kelvin.
Since DH° is negative and DS° is positive, the sign of DG° will depend on the temperature.
At high temperatures, the TDS° term dominates, making the reaction spontaneous. This is because the positive entropy change overcomes the negative enthalpy change, resulting in a negative DG°.
At low temperatures, the DH° term dominates, making the reaction nonspontaneous. This is because the negative enthalpy change overcomes the positive entropy change, resulting in a positive DG°.
Therefore, the reaction is spontaneous only at high temperatures and nonspontaneous at low temperatures.