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 44
As shown in Table 15.2, Kp for the equilibrium N2(g) + 3 H2(g) ⇌ 2 NH3(g) is 4.51 * 10^-5 at 450 _x001F_C. For each of the mixtures listed here, indicate whether the mixture is at equilibrium at 450 _x001F_C. If it is not at equilibrium, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. (a) 98 atm NH3, 45 atm N2, 55 atm H2. (b) 57 atm NH3, 143 atm N2, no H2. (c) 13 atm NH3, 27 atm N2, 82 atm H2.
검증된 단계별 안내1
Step 1: Write the expression for the equilibrium constant Kp for the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g). The expression is Kp = (P_{NH3}^2) / (P_{N2} * P_{H2}^3), where P represents the partial pressures of the gases.
Step 2: For each mixture, calculate the reaction quotient Qp using the same expression as Kp: Qp = (P_{NH3}^2) / (P_{N2} * P_{H2}^3). Substitute the given partial pressures into this expression for each case.
Step 3: Compare the calculated Qp value with the given Kp value (4.51 * 10^-5) for each mixture. This comparison will help determine the state of the system relative to equilibrium.
Step 4: If Qp = Kp, the system is at equilibrium. If Qp < Kp, the reaction will shift toward the products (right) to reach equilibrium. If Qp > Kp, the reaction will shift toward the reactants (left) to reach equilibrium.
Step 5: Analyze each mixture: (a) Calculate Qp and compare with Kp to determine the direction of shift. (b) Calculate Qp and compare with Kp to determine the direction of shift. (c) Calculate Qp and compare with Kp to determine the direction of shift.
주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Equilibrium Constant (Kp)
The equilibrium constant, Kp, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g), Kp is calculated using the partial pressures of the gases involved. A Kp value of 4.51 * 10^-5 indicates that at equilibrium, the concentration of reactants is much higher than that of the products, suggesting that the reaction favors the formation of reactants.
추천 영상:
가이드 코스
03:20
Equilibrium Constant Expressions
Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust to counteract that change and restore a new equilibrium. This principle helps predict the direction in which a reaction will shift when the concentrations of reactants or products are altered, allowing us to determine whether a mixture is at equilibrium or not.
추천 영상:
가이드 코스
07:32Le Chatelier's Principle
Reaction Quotient (Q)
The reaction quotient, Q, is calculated using the same formula as Kp but uses the current concentrations or partial pressures of the reactants and products, regardless of whether the system is at equilibrium. By comparing Q to Kp, one can determine the direction in which the reaction will shift: if Q < Kp, the reaction shifts toward products; if Q > Kp, it shifts toward reactants. This comparison is essential for assessing the state of the mixtures provided in the question.
추천 영상:
가이드 코스
00:49Reaction Quotient Q
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교과서 질문
At 900 K, the following reaction has 𝐾𝑝 = 0.345: 2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?
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교과서 질문
At 100°C, the equilibrium constant for the reaction COCl2(𝑔) ⇌ CO(𝑔) + Cl2(𝑔) has the value 𝐾𝑐 = 2.19×10−10. Are the following mixtures of COCl2, CO, and Cl2 at 100°C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.
(a) [COCl2] = 2.00×10−3 M, [CO] = 3.3×10−6 M, [Cl2] = 6.62×10−6 M
(b) [COCl2] = 4.50×10−2 M, [CO] = 1.1×10−7 M, [Cl2] = 2.25×10−6 M
(c) [COCl2] = 0.0100 M, [CO] = [Cl2] = 1.48×10−6 M
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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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