교과서 질문
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?
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Ch.15 - Chemical Equilibrium
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
15장, 문제 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).
검증된 단계별 안내1
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.
주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
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.
추천 영상:
가이드 코스
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.
추천 영상:
가이드 코스
01:14ICE 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.
추천 영상:
가이드 코스
07:32Le Chatelier's Principle