Skip to main content
Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.15 - Chemical EquilibriumProblema 43
Capitolo 15, Problema 43

Consider the reaction: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq). A solution is made containing an initial [Fe3+] of 1.0*10^-3 M and an initial [SCN-] of 8.0*10^-4 M. At equilibrium, [FeSCN2+] = 1.7*10^-4 M. Calculate the value of the equilibrium constant (Kc).

Guida verificata passo dopo passo
1
Identify the initial concentrations of the reactants: [Fe^{3+}]_0 = 1.0 \(\times\) 10^{-3} \(\text{ M}\) and [SCN^-]_0 = 8.0 \(\times\) 10^{-4} \(\text{ M}\).
Determine the change in concentration for the formation of FeSCN^{2+} at equilibrium, which is given as [FeSCN^{2+}] = 1.7 \(\times\) 10^{-4} \(\text{ M}\).
Calculate the equilibrium concentrations of the reactants: [Fe^{3+}]_{eq} = [Fe^{3+}]_0 - [FeSCN^{2+}] and [SCN^-]_{eq} = [SCN^-]_0 - [FeSCN^{2+}].
Write the expression for the equilibrium constant K_c: K_c = \(\frac{[FeSCN^{2+}\)]_{eq}}{[Fe^{3+}]_{eq} \(\times\) [SCN^-]_{eq}}.
Substitute the equilibrium concentrations into the K_c expression to find the value of the equilibrium constant.

Concetti chiave

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

Equilibrium Constant (Kc)

The equilibrium constant (Kc) 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 formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. A larger Kc indicates a greater concentration of products at equilibrium, while a smaller Kc suggests that reactants are favored.
Video consigliato:
Percorso guidato
03:20
Equilibrium Constant Expressions

ICE Table

An ICE table (Initial, Change, Equilibrium) is a tool used to organize the concentrations of reactants and products in a chemical reaction at different stages. It helps in determining the changes in concentration as the reaction progresses towards equilibrium. By filling in the initial concentrations, the changes that occur, and the equilibrium concentrations, one can easily calculate the equilibrium constant.
Video consigliato:
Percorso guidato
01:14
ICE Charts and Equilibrium Amount

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 understanding how changes in concentration, pressure, or temperature can affect the position of equilibrium and the value of the equilibrium constant.
Video consigliato:
Percorso guidato
07:32
Le Chatelier's Principle
Pratica correlata
Domanda del libro di testo

Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91⨉103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2in this mixture?

1673
views