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Ch.16 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.16 - Chemical EquilibriumProblema 68a
Capitolo 16, Problema 68a

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. a. CO(g) + H2O( g) ⇌ CO2(g) + H2(g) (volume is decreased)

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Identify the reaction and the change in conditions: The given reaction is CO(g) + H2O(g) ⇌ CO2(g) + H2(g), and the volume of the container is decreased.
Determine the change in the number of moles of gas on each side of the equation: On the left side, there are 2 moles of gas (1 mole of CO and 1 mole of H2O), and on the right side, there are also 2 moles of gas (1 mole of CO2 and 1 mole of H2).
Apply Le Chatelier's Principle: According to Le Chatelier's Principle, if the volume of a system at equilibrium is decreased, the system will shift in the direction that produces fewer moles of gas to counteract the change.
Compare the moles of gas on both sides: Since the number of moles of gas on both sides of the reaction is equal, decreasing the volume does not change the number of moles of gas produced.
Predict the effect of the volume change: Since the number of moles of gas remains the same on both sides, decreasing the volume will have no effect on the position of the 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. This principle helps predict how a system at equilibrium will respond to changes in concentration, temperature, or pressure.
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Le Chatelier's Principle

Effect of Volume Change on Gaseous Equilibria

In gaseous equilibria, a decrease in volume increases the pressure of the system. According to Le Chatelier's Principle, the equilibrium will shift toward the side with fewer moles of gas to reduce the pressure. Conversely, an increase in volume decreases pressure, shifting the equilibrium toward the side with more moles of gas.
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Constant-Volume Calorimetry

Stoichiometry of the Reaction

Understanding the stoichiometry of the reaction is crucial for predicting shifts in equilibrium. In the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g), there are 2 moles of gas on the left and 2 moles on the right. Since the number of moles is equal, a volume change will not favor either side, leading to no effect on the equilibrium position.
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Stoichiometry Concept
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