By calculating ΔH° and ΔS° for the balanced reaction 3O2(g) ⇌ 2O3(g), and making
use of only the algebraic signs of these quantities, deduce whether spontaneity or nonspontaneity
of ozone formation from oxygen is influenced by temperature.
Explain your answ
To determine the influence of temperature on the spontaneity or non-spontaneity of the ozone formation reaction, we need to analyze the signs of the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°) for the reaction.
The reaction given is: 3O2(g) ⇌ 2O3(g)
1. Enthalpy Change (ΔH°):
- If ΔH° is negative (-), it means the reaction is exothermic, releasing heat during the formation of products.
- If ΔH° is positive (+), it means the reaction is endothermic, absorbing heat during the formation of products.
2. Entropy Change (ΔS°):
- If ΔS° is positive (+), it means the reaction leads to an increase in disorder or randomness of particles.
- If ΔS° is negative (-), it means the reaction leads to a decrease in disorder or randomness of particles.
Now, let's consider the two scenarios:
1. ΔH° < 0 and ΔS° > 0:
In this case, the reaction is exothermic and leads to an increase in disorder. This combination suggests that increasing the temperature will favor the formation of ozone from oxygen. The reaction is spontaneous at higher temperatures.
2. ΔH° > 0 and ΔS° < 0:
In this case, the reaction is endothermic and leads to a decrease in disorder. This combination suggests that increasing the temperature will unfavor the formation of ozone from oxygen. The reaction is non-spontaneous at higher temperatures.
In conclusion, the spontaneity of ozone formation from oxygen is influenced by temperature. If the reaction is exothermic and leads to an increase in disorder, increasing the temperature will make the reaction more spontaneous. On the other hand, if the reaction is endothermic and leads to a decrease in disorder, increasing the temperature will make the reaction less spontaneous.