What is AS at 298 K for the following reaction? Fe2O3(s) + 3CO(g) - 3CO2(g) + 2Fe(s) Substance AGf(kJ/mol) AHf(kJ/mol) Fe2O3(s) CO(g) CO2(g) -741.0 -137.2 -394.4 -822.2 -110.5 -393.5

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**Calculating ΔS° at 298 K for a Chemical Reaction**

This section explains how to determine the standard entropy change (ΔS°) at 298 K for the following chemical reaction:

\[ \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 3\text{CO}_2(g) + 2\text{Fe}(s) \]

The table below provides the standard Gibbs free energy of formation (ΔG°f) and standard enthalpy of formation (ΔH°f) in kilojoules per mole (kJ/mol) for each substance involved in the reaction:

| Substance   | ΔG°f (kJ/mol) | ΔH°f (kJ/mol) |
|-------------|---------------|---------------|
| Fe₂O₃(s)    | -741.0        | -822.2        |
| CO(g)       | -137.2        | -110.5        |
| CO₂(g)      | -394.4        | -393.5        |

To calculate ΔS°, use the formula relating Gibbs free energy, enthalpy, and entropy:

\[ ΔG° = ΔH° - TΔS° \]

where \( ΔG° \) is the standard Gibbs free energy change, \( ΔH° \) is the standard enthalpy change, and \( T \) is the temperature in Kelvin.

By calculating these thermodynamic values for the entire reaction, we can determine the change in entropy (ΔS°) at the specified temperature.
Transcribed Image Text:**Calculating ΔS° at 298 K for a Chemical Reaction** This section explains how to determine the standard entropy change (ΔS°) at 298 K for the following chemical reaction: \[ \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 3\text{CO}_2(g) + 2\text{Fe}(s) \] The table below provides the standard Gibbs free energy of formation (ΔG°f) and standard enthalpy of formation (ΔH°f) in kilojoules per mole (kJ/mol) for each substance involved in the reaction: | Substance | ΔG°f (kJ/mol) | ΔH°f (kJ/mol) | |-------------|---------------|---------------| | Fe₂O₃(s) | -741.0 | -822.2 | | CO(g) | -137.2 | -110.5 | | CO₂(g) | -394.4 | -393.5 | To calculate ΔS°, use the formula relating Gibbs free energy, enthalpy, and entropy: \[ ΔG° = ΔH° - TΔS° \] where \( ΔG° \) is the standard Gibbs free energy change, \( ΔH° \) is the standard enthalpy change, and \( T \) is the temperature in Kelvin. By calculating these thermodynamic values for the entire reaction, we can determine the change in entropy (ΔS°) at the specified temperature.
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