Domanda del libro di testo
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(𝑔) + 2 H2(𝑔) ⇌ CH3OH(𝑔) (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature?
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Ch.15 - Chemical Equilibrium
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 15, Problema 66c
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(𝑔) + 2 H2(𝑔) ⇌ CH3OH(𝑔) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?
Guida verificata passo dopo passo1
Understand the concept of Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
Identify the number of moles of gas on both sides of the reaction: 1 mole of CO and 2 moles of H2 on the left (total 3 moles) and 1 mole of CH3OH on the right.
Recognize that increasing the pressure of a system in equilibrium favors the side of the reaction with fewer moles of gas. In this reaction, the right side with CH3OH has fewer moles of gas compared to the left side.
Conclude that to maximize the equilibrium yield of methanol, a high pressure should be used because it will shift the equilibrium towards the formation of methanol, which has fewer moles of gas.
Consider other factors that might affect the yield, such as temperature and catalysts, but for pressure specifically, a high pressure is favorable for increasing the yield of methanol in this reaction.
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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, increasing pressure favors the side of the reaction with fewer moles of gas, while decreasing pressure favors the side with more moles.
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Percorso guidato
07:32
Le Chatelier's Principle
Mole Ratio in Reactions
In the given reaction, the mole ratio of reactants to products is crucial for understanding how pressure affects equilibrium. The reaction CO(g) + 2 H2(g) ⇌ CH3OH(g) has three moles of gas on the reactant side and one mole on the product side, indicating that increasing pressure will favor the formation of methanol.
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Percorso guidato
02:14Neutron-Proton Ratio
Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of concentrations of products to reactants at equilibrium. Changes in pressure can influence the concentrations of gaseous reactants and products, thereby affecting the position of equilibrium and the yield of methanol. A higher pressure shifts the equilibrium towards the side with fewer gas moles, potentially increasing K for the product.
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Percorso guidato
01:14Equilibrium Constant K
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