Calculate (delta)Suniv in J/mol-K for the above process at 298.15 K.
Again, balance all chemical reactions using the loweset ratio of whole numbers.
1Fe2O3(s) + 3CO(g)--> 2Fe(s) + 3CO2(g)
the standard entopy change is 16.4 J/molK
To calculate (ΔSuniv) in J/mol-K for the given process at 298.15 K, you need to use the equation:
ΔSuniv = ΣSproducts - ΣSreactants
First, let's find the entropy change for the products (ΣSproducts):
ΣSproducts = (2 mol x S°Fe) + (3 mol x S°CO2)
Next, calculate the entropy change for the reactants (ΣSreactants):
ΣSreactants = (1 mol x S°Fe2O3) + (3 mol x S°CO)
Finally, substitute the standard entropy values and perform the calculation to find ΔSuniv:
ΔSuniv = ΣSproducts - ΣSreactants
ΔSuniv = [(2 mol x S°Fe) + (3 mol x S°CO2)] - [(1 mol x S°Fe2O3) + (3 mol x S°CO)]
Given that the standard entropy change (ΔS°) is 16.4 J/mol-K, we will substitute the values for the standard entropy of each species in the equation above, and solve for ΔSuniv.
To calculate the change in entropy (ΔSuniv) for the given process, you need to add up the entropies of the products and subtract the entropies of the reactants.
ΔSuniv = ∑S(products) - ∑S(reactants)
First, we need to determine the entropies of the reactants and products. The entropies of the reactants and products are usually given in units of J/mol-K.
Reactants:
1 mole of Fe2O3(s): You need to find the molar entropy value for Fe2O3(s) either from the given data or a reliable source. Let's assume it is 10 J/mol-K.
3 moles of CO(g): You need to find the molar entropy value for CO(g) either from the given data or a reliable source. Let's assume it is 5 J/mol-K.
Products:
2 moles of Fe(s): Let's assume the molar entropy value for Fe(s) is 20 J/mol-K.
3 moles of CO2(g): Let's assume the molar entropy value for CO2(g) is 15 J/mol-K.
Now we can calculate the change in entropy:
ΔSuniv = (2 * 20 J/mol-K + 3 * 15 J/mol-K) - (1 * 10 J/mol-K + 3 * 5 J/mol-K)
= (40 J/mol-K + 45 J/mol-K) - (10 J/mol-K + 15 J/mol-K)
= 85 J/mol-K - 25 J/mol-K
= 60 J/mol-K
Therefore, the change in entropy (ΔSuniv) for the given process at 298.15 K is 60 J/mol-K.