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
delta Srxn = (n*DSproducts)-(n*DSreactants)
To calculate ΔS (change in entropy) for the given reaction, you need to use the formula:
ΔS = ΣnS(products) - ΣmS(reactants)
Where:
- ΔS is the change in entropy
- ΣnS(products) is the sum of the entropy of the products, multiplied by their stoichiometric coefficients (n)
- ΣmS(reactants) is the sum of the entropy of the reactants, multiplied by their stoichiometric coefficients (m)
Given the stoichiometric coefficients and entropy values, let's substitute the values into the formula.
ΔS = (4 × 42.6 J/mol·K) + (1 × 205.2 J/mol·K) - (2 × 121.3 J/mol·K)
Calculate each term:
ΔS = 170.4 J/mol·K + 205.2 J/mol·K - 242.6 J/mol·K
Now, perform the addition and subtraction:
ΔS = 132.8 J/mol·K
Therefore, the change in entropy (ΔS) for the given reaction is 132.8 J/mol·K.