Use the data in Appendix 4 for the following. a. Calculate ΔH^∘ and ΔS^∘ for the reaction 3 Fe2

step 1 Now the delta h in this function is as 2 minus 117 plus minus 39 3 .5 minus 36 minus 8 26 plus m

Use the data in Appendix 4 for the following. a. Calculate...

Use the data in Appendix 4 for the following. a. Calculate $\Delta H^{\circ}$ and $\Delta S^{\circ}$ for the reaction $$3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g)$$ that occurs in a blast furnace. b. Assume that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ are independent of temperature. Calculate $\Delta G^{\circ}$ at $800 .{ }^{\circ} \mathrm{C}$ for this reaction.

Use the data in Appendix 4 for the following.
a. Calculate $\Delta H^{\circ}$ and $\Delta S^{\circ}$ for the reaction
$$3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g)$$
that occurs in a blast furnace.
b. Assume that $\Delta H^{\circ}$ and $\Delta S^{\circ}$ are independent of temperature. Calculate $\Delta G^{\circ}$ at $800 .{ }^{\circ} \mathrm{C}$ for this reaction.

Key Concepts

Temperature Independence Assumption

Assuming that ?H° and ?S° are constant over a temperature range simplifies calculations and predictions about a reaction’s Gibbs free energy. This approximation is often used when the temperature range is limited, allowing one to apply the relationship between enthalpy, entropy, and temperature to estimate reaction spontaneity at various temperatures.

Gibbs Free Energy Change (?G°)

This thermodynamic quantity combines the effects of enthalpy and entropy to predict the spontaneity of a chemical reaction under constant temperature and pressure. The relationship ?G° = ?H° - T?S° allows one to assess whether a reaction will proceed spontaneously (?G° < 0) or not (?G° > 0), essential for understanding chemical equilibria.

Standard Enthalpy Change (?H°)

This concept represents the heat absorbed or released during a chemical reaction at standard conditions. It is calculated as the difference between the enthalpy of the products and the enthalpy of the reactants, and is used to determine whether a reaction is endothermic or exothermic, a critical part of understanding reaction energetics.

Standard Entropy Change (?S°)

This is a measure of the change in disorder or randomness in a system as a result of a chemical reaction. It is determined by calculating the difference between the entropy of the products and the entropy of the reactants, reflecting how energy disperses at the molecular level, which plays an important role in predicting reaction spontaneity.

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