교과서 질문
(a) If Qc > Kc, how must the reaction proceed to reach equilibrium?
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Ch.15 - Chemical Equilibrium
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
15장, 문제 41a
(a) If Qc < Kc, in which direction will a reaction proceed in order to reach equilibrium?
검증된 단계별 안내1
Identify the given terms: Q_c is the reaction quotient, and K_c is the equilibrium constant.
Understand the relationship: If Q_c < K_c, it means the concentration of products is less than what is required at equilibrium.
Determine the direction: The reaction will proceed in the forward direction to produce more products and reach equilibrium.
Visualize the process: As the reaction moves forward, the concentration of reactants will decrease, and the concentration of products will increase.
Conclude the reasoning: The reaction continues in the forward direction until Q_c equals K_c, achieving equilibrium.
비슷한 문제에 대한 검증된 영상 답변:
이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
1m주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Reaction Quotient (Q<sub>c</sub>)
The reaction quotient, Q<sub>c</sub>, is a measure of the relative concentrations of products and reactants at any point in a reaction. It is calculated using the same expression as the equilibrium constant (K<sub>c</sub>), but with the current concentrations instead of equilibrium concentrations. Q<sub>c</sub> helps determine the direction in which a reaction will shift to reach equilibrium.
추천 영상:
가이드 코스
00:49
Reaction Quotient Q
Equilibrium Constant (K<sub>c</sub>)
The equilibrium constant, K<sub>c</sub>, is a value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is a fixed value for a particular reaction under specified conditions. Comparing Q<sub>c</sub> to K<sub>c</sub> allows us to predict the direction of the reaction's shift towards equilibrium.
추천 영상:
가이드 코스
01:14Equilibrium Constant K
Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. In the context of Q<sub>c</sub> and K<sub>c</sub>, if Q<sub>c</sub> is less than K<sub>c</sub>, the reaction will shift to the right, favoring the formation of products to achieve equilibrium.
추천 영상:
가이드 코스
07:32Le Chatelier's Principle
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교과서 질문
A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) (d) Calculate Kc for the reaction.
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교과서 질문
(b) At the start of a certain reaction, only reactants are present; no products have been formed. What is the value of Qc at this point in the reaction?
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교과서 질문
(b) What condition must be satisfied so that Qc = Kc?
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