This question is about thermodynamics. Consider the reaction shown below:
2Fe2O3(s)+3C(s)→4Fe(s)+3CO2(g) 2\text{Fe}_2\text{O}_3(\text{s}) + 3\text{C}(\text{s}) \rightarrow 4\text{Fe}(\text{s}) + 3\text{CO}_2(\text{g}) 2Fe2O3(s)+3C(s)→4Fe(s)+3CO2(g)The table below shows some thermodynamic data.
| Substance | Fe2O3(s)\text{Fe}_2\text{O}_3(\text{s})Fe2O3(s) | Fe(s)\text{Fe}(\text{s})Fe(s) | C(s)\text{C}(\text{s})C(s) | CO2(g)\text{CO}_2(\text{g})CO2(g) |
|---|---|---|---|---|
| ΔfH⊖ / kJ mol−1\Delta_f H^\ominus\ /\ \text{kJ mol}^{-1}ΔfH⊖ / kJ mol−1 | −824-824−824 | 000 | 000 | −394-394−394 |
| S⊖ / J K−1mol−1S^\ominus\ /\ \text{J K}^{-1}\text{mol}^{-1}S⊖ / J K−1mol−1 | 878787 | 272727 | 666 | 214214214 |
Explain why the standard entropy value for carbon dioxide is greater than that for carbon.
State the temperature at which the standard entropy of iron is 0 J K−1mol−10\ \text{J K}^{-1}\text{mol}^{-1}0 J K−1mol−1.
Use the equation and the thermodynamic data provided to calculate the minimum temperature, in K\text{K}K, at which this reaction becomes feasible.
