Skip to main content
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 29c
Capitolo 16, Problema 29c

This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
c. 2 CH3OH(g) ⇌ 2 CO(g) + 4 H2(g)

Guida verificata passo dopo passo
1
Identify the relationship between the given reaction and the reaction in part c. The reaction in part c is the reverse of the given reaction, and it is also multiplied by a factor of 2.
Recall that the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction. Mathematically, if the forward reaction has an equilibrium constant K, then the reverse reaction has an equilibrium constant of 1/K.
Since the reaction in part c is also multiplied by 2, remember that when a reaction is multiplied by a factor, the equilibrium constant is raised to the power of that factor. If a reaction is multiplied by n, then the new equilibrium constant K' = K^n.
Apply these principles to calculate the new equilibrium constant Kp for the reaction in part c. Use the formula Kp' = (1/Kp)^2, where Kp is the equilibrium constant of the original reaction.
Predict whether reactants or products will be favored at equilibrium by comparing the magnitude of Kp' to 1. If Kp' > 1, products are favored; if Kp' < 1, reactants are favored.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
1m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the partial pressures of gases involved in the reaction. A larger Kp value indicates that products are favored at equilibrium, while a smaller Kp suggests that reactants are favored.
Video consigliato:
Percorso guidato
03:20
Equilibrium Constant Expressions

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 helps predict the direction in which a reaction will shift when changes in concentration, pressure, or temperature occur, thus influencing the favorability of reactants or products.
Video consigliato:
Percorso guidato
07:32
Le Chatelier's Principle

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, as represented by the balanced chemical equation. Understanding stoichiometry is essential for calculating equilibrium constants for different reactions, as it allows for the proper adjustment of coefficients when deriving Kp for reactions that differ from the original equation.
Video consigliato:
Percorso guidato
01:16
Stoichiometry Concept
Pratica correlata
Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 6 COF2(g) ⇌ 3 CO2(g) + 3 CF4(g)

713
views
Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium. a. CH3OH(g) ⇌ CO(g) + 2 H2(g)

790
views
Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

c. 2 CO2(g) + 2 CF4(g) ⇌ 4 COF2(g)

631
views
Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

a. COF2 (g) ⇌ 1/2 CO2(g) + 1/2 CF4(g)

2676
views
1
comments
Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 1/2 CO(g) + H2 (g) ⇌ 1/2 CH3OH(g)

3230
views
Domanda del libro di testo

A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2⨉104 at room temperature. However, upon carrying out both reactions for 15 minutes, the chemist finds that the reaction with the smaller equilibrium constant produces more of the desired product. Explain how this might be possible.

1175
views