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Ch.5 - Thermochemistry
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.5 - ThermochemistryProblema 66
Capitolo 5, Problema 66

Given the data N2(g) + O2(g) → 2 NO(g) ΔH = +180.7 kJ 2 NO(g) + O2(g) → 2 NO2(g) ΔH = -113.1 kJ 2 N2O(g) → 2 N2(g) + O2(g) ΔH = -163.2 kJ use Hess's law to calculate ΔH for the reaction N2O(g) + NO2(g) → 3 NO(g)

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Identify the target reaction: \( \text{N}_2\text{O}(g) + \text{NO}_2(g) \rightarrow 3 \text{NO}(g) \).
Write down the given reactions and their enthalpy changes: \( \text{N}_2(g) + \text{O}_2(g) \rightarrow 2 \text{NO}(g) \), \( \Delta H = +180.7 \text{ kJ} \); \( 2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \), \( \Delta H = -113.1 \text{ kJ} \); \( 2 \text{N}_2\text{O}(g) \rightarrow 2 \text{N}_2(g) + \text{O}_2(g) \), \( \Delta H = -163.2 \text{ kJ} \).
Reverse the third reaction to match the target reaction's reactants: \( 2 \text{N}_2(g) + \text{O}_2(g) \rightarrow 2 \text{N}_2\text{O}(g) \), changing \( \Delta H \) to \(+163.2 \text{ kJ} \).
Adjust the stoichiometry of the reactions to match the target reaction: Divide the first reaction by 2 to get \( \text{N}_2(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{NO}(g) \), and divide the second reaction by 2 to get \( \text{NO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{NO}_2(g) \).
Combine the adjusted reactions to form the target reaction, ensuring that the intermediates cancel out, and sum the enthalpy changes to find \( \Delta H \) for the target reaction.

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Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the sum of the enthalpy changes for the individual steps of the reaction, regardless of the pathway taken. This principle allows chemists to calculate the enthalpy change for a reaction that may be difficult to measure directly by using known enthalpy changes of related reactions.
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Hess's Law

Enthalpy Change (ΔH)

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ΔH < 0) or endothermic (absorbs heat, ΔH > 0). Understanding ΔH is crucial for predicting the energy changes associated with chemical reactions and for applying Hess's Law effectively.
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Enthalpy of Formation

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It is essential for determining the proportions of substances involved in reactions, which is necessary when applying Hess's Law to combine multiple reactions and find the overall enthalpy change for a target reaction.
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Stoichiometry Concept
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