Domanda del libro di testo
Consider this reaction at equilibrium: 2 BrNO(g) ⇌ 2 NO(g) + Br2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. b. BrNO is added to the reaction mixture.
773
views
Ch.16 - Chemical Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 63
Consider the reaction: A(g) ⇌ B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. b. Kc = 0.010
Guida verificata passo dopo passo1
Step 1: Define the initial concentrations of the reactants and products. For A, the initial concentration is 1.0 M, and for B and C, the initial concentrations are 0 M.
Step 2: Set up the change in concentrations that occurs as the system reaches equilibrium. Let x be the amount of A that reacts to form B and C. At equilibrium, the concentration of A will be (1.0 - x) M, and the concentrations of B and C will each be x M.
Step 3: Write the expression for the equilibrium constant, Kc, in terms of the concentrations of the reactants and products at equilibrium. For the reaction A ⇌ B + C, the expression is Kc = \(\frac{[B][C]}{[A]}\) = \(\frac{x^2}{1.0 - x}\).
Step 4: Substitute the given value of Kc into the equilibrium expression and solve for x. In this case, Kc = 0.010, so set up the equation 0.010 = \(\frac{x^2}{1.0 - x}\).
Step 5: Solve the quadratic equation derived in step 4 for x to find the equilibrium concentrations of A, B, and C. The equilibrium concentration of A will be 1.0 - x, and the concentrations of B and C will each be x.
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:
8mConcetti 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 state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in concentration. Understanding this concept is crucial for analyzing how concentrations shift in response to changes in conditions or equilibrium constants.
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, each raised to the power of their coefficients in the balanced equation. A small Kc value, such as 0.010, indicates that at equilibrium, the concentration of reactants is much greater than that of products, suggesting that the reaction favors the reactants. This concept is essential for predicting the direction of the reaction and the concentrations of species at equilibrium.
Video consigliato:
Percorso guidato
03:20Equilibrium Constant Expressions
ICE Table (Initial, Change, Equilibrium)
An ICE table is a tool used to organize the initial concentrations, the changes in concentrations as the reaction proceeds, and the equilibrium concentrations of reactants and products. By setting up an ICE table, one can systematically determine how the concentrations of A, B, and C change in response to the reaction and the given Kc value. This method simplifies the calculation process and helps visualize the relationship between the species involved in the reaction.
Video consigliato:
Percorso guidato
01:14ICE Charts and Equilibrium Amount
Pratica correlata
Domanda del libro di testo
Consider this reaction at equilibrium: 2 BrNO(g) ⇌ 2 NO(g) + Br2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. NO is added to the reaction mixture.
815
views
Domanda del libro di testo
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99⨉10-7 at 227 °C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?
2819
views
Domanda del libro di testo
Consider the reaction: HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Kc = 1.8⨉10-5 at 25°C If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 °C?
3717
views