Skip to main content
Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 74a
Capitolo 15, Problema 74a

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.

Guida verificata passo dopo passo
1
Determine the initial concentration of SO2Cl2 by dividing the number of moles by the volume of the flask. This gives the initial concentration in moles per liter.
Calculate the change in concentration of SO2Cl2 due to decomposition. Since 56% decomposes, multiply the initial concentration by 0.56 to find the amount that decomposed.
Write the expression for the equilibrium constant, Kc, for the reaction: Kc = \( \frac{[SO_2][Cl_2]}{[SO_2Cl_2]} \).
At equilibrium, the concentration of SO2 and Cl2 will be equal to the amount of SO2Cl2 that decomposed, and the concentration of SO2Cl2 will be the initial concentration minus the amount that decomposed.
Substitute the equilibrium concentrations into the Kc expression and solve for Kc.

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:
7m

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 this context, the decomposition of SO2Cl2 into SO2 and Cl2 reaches a state where the amounts of each species remain unchanged over time, allowing for the calculation of the equilibrium constant, Kc.
Video consigliato:
Percorso guidato
04:21
Chemical Equilibrium Concepts

Equilibrium Constant (Kc)

The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium, raised to the power of their stoichiometric coefficients. For the reaction SO2Cl2 ⇌ SO2 + Cl2, Kc is calculated using the formula Kc = [SO2][Cl2] / [SO2Cl2], where the brackets denote molarity. This constant provides insight into the extent of the reaction and the favorability of product formation.
Video consigliato:
Percorso guidato
03:20
Equilibrium Constant Expressions

Molarity and Concentration Calculations

Molarity is defined as the number of moles of solute per liter of solution, expressed as M = moles/volume. In this problem, the initial concentration of SO2Cl2 is determined by dividing the moles (2.00 mol) by the volume of the flask (2.00 L), which is essential for calculating the equilibrium concentrations after accounting for the decomposition of the reactant.
Video consigliato:
Percorso guidato
03:12
Molar Mass Calculation Example
Pratica correlata
Domanda del libro di testo

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (c) According to Le Châtelier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

557
views