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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 62f
Capitolo 15, Problema 62f

Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) ⇌ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = −904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.

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Identify the type of reaction: The given reaction is exothermic, as indicated by the negative \( \Delta H = -904.4 \) kJ.
Apply Le Chatelier's Principle: In an exothermic reaction, increasing the temperature will shift the equilibrium position to favor the endothermic direction, which is the reverse reaction in this case.
Determine the effect on NO yield: Since the equilibrium shifts towards the reactants (reverse reaction), the yield of NO will decrease.
Consider the overall impact: Increasing temperature in an exothermic reaction generally decreases the yield of products formed in the forward reaction.
Conclude: Therefore, increasing the temperature will decrease the yield of NO at equilibrium.

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Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of temperature changes, if the reaction is exothermic (releases heat), increasing the temperature will shift the equilibrium to favor the reactants, thereby decreasing the yield of products.
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Le Chatelier's Principle

Exothermic Reactions

An exothermic reaction is one that releases energy in the form of heat. In the given reaction, the negative ΔH value indicates that it is exothermic. When the temperature is increased, the system will respond by favoring the endothermic direction (the reverse reaction) to absorb the added heat, which reduces the production of NO.
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Endothermic & Exothermic Reactions

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in temperature can alter the value of K, affecting the position of equilibrium. For exothermic reactions, increasing temperature decreases K, leading to a lower concentration of products like NO at equilibrium.
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Equilibrium Constant K
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