Skip to main content
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 38
Capitolo 16, Problema 38

Consider the following reaction: H2(g) + I2(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.
T (°C) [H2] [I2] [HI] Kc
25 0.0355 0.0388 0.922 _
340 _ 0.0455 0.387 9.6
445 0.0485 0.0468 _ 50.2

Guida verificata passo dopo passo
1
Identify the balanced chemical equation for the reaction: H2(g) + I2(g) ⇌ 2 HI(g).
Use the equilibrium constant expression for the reaction, Kc = \(\frac{[HI]^2}{[H2][I2]}\), to set up the equation for each scenario provided in the table.
For each row in the table, substitute the given equilibrium concentrations of H2, I2, and HI into the Kc expression.
Calculate Kc by solving the expression for each set of concentrations. Remember to square the concentration of HI since it has a coefficient of 2 in the balanced equation.
Ensure the units are consistent and that all concentrations are in moles per liter (M) before substituting them into the Kc expression.

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:
2m

Concetti chiave

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

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the given reaction, H2 and I2 combine to form HI, and at equilibrium, the concentrations of all species remain unchanged over time. Understanding this concept is crucial for analyzing the provided equilibrium concentrations and calculating the equilibrium constant (Kc).
Video consigliato:
Percorso guidato
04:21
Chemical Equilibrium Concepts

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. For the reaction H2(g) + I2(g) ⇌ 2 HI(g), Kc is calculated as [HI]^2 / ([H2][I2]). This constant provides insight into the position of equilibrium and how it shifts with changes in concentration or temperature.
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 to counteract the change and restore a new equilibrium. This principle helps predict how changes in temperature, pressure, or concentration will affect the equilibrium position of the reaction. In the context of the question, understanding this principle is essential for interpreting how Kc values might vary with temperature.
Video consigliato:
Percorso guidato
07:32
Le Chatelier's Principle
Pratica correlata
Domanda del libro di testo

Consider the reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.

T (K) [N2] [H2] [NH3] Kc

500 0.115 0.105 0.439 _

575 0.110 _ 0.128 9.6

775 0.120 0.140 _ 0.0584

764
views
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
Domanda del libro di testo

Consider the reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) Kp = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture?

1820
views