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Ch.16 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.16 - Chemical EquilibriumProblema 72c
Capitolo 16, Problema 72c

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. c. CaCO3(s) ⇌ CaO(s) + CO2(g) (volume is increased)

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Identify the reaction type: The given reaction is a decomposition reaction where solid calcium carbonate (CaCO3) decomposes into solid calcium oxide (CaO) and gaseous carbon dioxide (CO2).
Determine the effect of volume change on gases: Increasing the volume of the system decreases the pressure. According to Le Chatelier's principle, the system will adjust to counteract this change.
Analyze the reaction's response to pressure change: In this reaction, the only gaseous product is CO2. Increasing the volume (and thus decreasing the pressure) will shift the equilibrium towards the side with more moles of gas.
Count the moles of gases on each side of the equation: The reactant side has no gaseous moles, and the product side has one mole of CO2 gas.
Predict the shift in equilibrium: Since increasing the volume favors the formation of more gas, the equilibrium will shift to the right, promoting the decomposition of CaCO3 to form more CO2.

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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 system will adjust itself to counteract the change and restore a new equilibrium. This principle is crucial for predicting how a system will respond to changes in concentration, temperature, or pressure.
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Le Chatelier's Principle

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. For gaseous reactions, changes in volume affect the partial pressures of the gases involved, which in turn influences the position of equilibrium.
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Equilibrium Constant K

Effect of Volume Change on Gaseous Equilibria

In reactions involving gases, increasing the volume decreases the pressure. According to Le Chatelier's Principle, the equilibrium will shift toward the side with more moles of gas to counteract the decrease in pressure. In the given reaction, the products side has one mole of gas (CO2), while the reactants side has none, indicating a shift to the right when volume is increased.
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Constant-Volume Calorimetry
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