The main distinction between enthalpy and entropy, which exists despite the fact that they are both components of a thermodynamic system, is that enthalpy is represented as the total amount of heat content while entropy is the level of disorder.
SO₂ (g) + 2H₂S (g) ⇄ 3S(s) + 2H₂O (g)
The standard ΔG and ΔH of the products less the standard ΔG and ΔH of the reactants may be used to calculate the ΔG and ΔH of the reaction. So, the reaction's ΔG is:
ΔGr = 3ΔG S(s) + 2ΔG H₂O (g) - ( ΔG SO₂ (g) + 2ΔG H₂S (g))
ΔGr = 3×0 kJ/mol + 2×-228,6 kJ/mol - (-300,4 kJ/mol + 2×-33,01 kJ/mol)
ΔGr = -90,78 kJ/mol
In the same way, ΔHr is:
ΔHr = ΔH S(s) + 2ΔH H₂O (g) - ( ΔH SO₂ (g) + 2ΔH H₂S (g))
ΔHr = 3×0 kJ/mol + 2×-241,8 kJ/mol - (-296,9 kJ/mol + 2×-20,17 kJ/mol)
ΔHr = -146,36 kJ/mol
A ΔH < 0 indicates that heat is being produced by the process. According to Le Chatelier's principle, which states that changes in a system's temperature, pressure, volume, or concentration will result in predictable and opposing changes in the system, raising the temperature will result in the production of less product, while lowering the temperature will result in the production of more product.
As 2 moles of gas produce 5 moles of gas if the pressure decreases the system will try to produce more gas opposing the change, and again if the pressure increases the system will try to produce less gas.
complete Question :
using relative enthalpy and entropy values, determine how the process is affected after each of the following temperature or pressure changes? consider that a more effective reaction produces more product or more product in a shorter amount of time.
Reaction: SO₂ (g) + 2H₂S (g) ↔ 3S(s) + 2H₂O (g)Substance | ΔG kJ/mol | ΔH kJ/molH₂O(g) | -228.6 | -241.8H₂O(l) | -237.1 | -285.8SO₂(g) | -300.4 | -296.9SO₃(g) | -370.4 | -395.2H₂S(g) | -33.01 | -20.17S(s) | 0 | 0Categorize into: "More Effective" ~ "Less Effective" ~ "Equally Effective"
To learn more about enthalpy and entropy refer,
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