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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 62d
Capitolo 15, Problema 62d

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? (d) decrease the volume of the container in which the reaction occurs

Guida verificata passo dopo passo
1
Identify the reaction type: The given reaction is an exothermic reaction, as indicated by the negative \( \Delta H \) value.
Apply Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Consider the effect of volume change: Decreasing the volume of the container increases the pressure of the system.
Analyze the reaction's response to pressure change: The reaction will shift towards the side with fewer moles of gas to reduce the pressure.
Count the moles of gas on each side: The left side has 9 moles (4 NH\(_3\) + 5 O\(_2\)), and the right side has 10 moles (4 NO + 6 H\(_2\)O). Therefore, decreasing the volume will shift the equilibrium towards the left, decreasing the yield of NO.

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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 gas reactions, reducing the volume of the container increases the pressure, prompting the equilibrium to shift toward the side with fewer moles of gas to alleviate the pressure increase.
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Le Chatelier's Principle

Mole Ratio in Reactions

In chemical reactions, the mole ratio indicates the proportion of reactants and products involved. For the given reaction, there are 9 moles of gas on the reactant side (4 NH₃ + 5 O₂) and 10 moles on the product side (4 NO + 6 H₂O). Understanding this ratio is crucial for predicting how changes in volume affect the equilibrium position.
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Neutron-Proton Ratio

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium. Changes in conditions, such as volume or temperature, can affect K. In this reaction, decreasing the volume increases the concentration of gases, which can shift the equilibrium position, thereby affecting the yield of NO.
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Equilibrium Constant K
Pratica correlata
Domanda del libro di testo

Consider the following equilibrium, for which Δ𝐻<0

2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)

(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(𝑔) is removed from the system?

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Domanda del libro di testo

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? (e) add a catalyst

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Domanda del libro di testo

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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Domanda del libro di testo

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? (a) increase [NH3] (b) increase [H2O] (c) decrease [O2]

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Domanda del libro di testo

Consider the following equilibrium, for which Δ𝐻<0

2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)

(e) the total pressure of the system is increased by adding a noble gas