Given the following data at 298K, calculate delta S for :
2Ag2O(s) -> 4Ag(s) +O2(g)
deltaS(J/mol.K)121.3 42.6 205.2
See your post above.
To calculate the change in entropy (ΔS) for the given reaction, you need to use the formula:
ΔS = ΣnS(products) - ΣnS(reactants)
Where:
- ΣnS(products) is the sum of the products' entropy, multiplied by their stoichiometric coefficient.
- ΣnS(reactants) is the sum of the reactants' entropy, multiplied by their stoichiometric coefficient.
In the given reaction: 2Ag2O(s) → 4Ag(s) + O2(g)
The stoichiometric coefficients are 2 for Ag2O(s), 4 for Ag(s), and 1 for O2(g).
Now, calculate ΔS using the provided entropy values (in J/mol.K):
ΔS = (4 * 42.6 J/mol.K) + (1 * 205.2 J/mol.K) - (2 * 121.3 J/mol.K)
= 170.4 J/mol.K + 205.2 J/mol.K - 242.6 J/mol.K
= 133 J/mol.K
Therefore, the change in entropy (ΔS) for the reaction 2Ag2O(s) → 4Ag(s) + O2(g) at 298K is 133 J/mol.K.