Domanda del libro di testo
At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br2(𝑔)?
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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
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 15, Problema 52
For the equilibrium Br2(𝑔) + Cl2(𝑔) ⇌ 2 BrCl(𝑔) at 400 K, 𝐾𝑐 = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?
Guida verificata passo dopo passo1
Identify the initial concentrations of Br_2 and Cl_2 by dividing the moles by the volume of the container: [Br_2]_0 = \(\frac{0.25 \text{ mol}\)}{3.0 \(\text{ L}\)}, [Cl_2]_0 = \(\frac{0.55 \text{ mol}\)}{3.0 \(\text{ L}\)}.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations as the system reaches equilibrium. Let x be the change in concentration of Br_2 and Cl_2 that reacts to form BrCl.
Write the expression for the equilibrium constant K_c: K_c = \(\frac{[BrCl]^2}{[Br_2][Cl_2]}\).
Substitute the equilibrium concentrations from the ICE table into the K_c expression: K_c = \(\frac{(2x)^2}{([Br_2]_0 - x)([Cl_2]_0 - x)}\).
Solve the equation for x, which represents the change in concentration, and use it to find the equilibrium concentrations: [Br_2] = [Br_2]_0 - x, [Cl_2] = [Cl_2]_0 - x, [BrCl] = 2x.
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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, such as concentration or temperature.
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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. For the reaction Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) ⇌ 2 BrCl(g), Kc = [BrCl]<sup>2</sup> / ([Br<sub>2</sub>][Cl<sub>2</sub>]). This constant provides insight into the extent of the reaction and helps predict the direction in which the reaction will shift to reach equilibrium.
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03:20Equilibrium Constant Expressions
Concentration Calculations
Concentration calculations involve determining the molarity of substances in a solution, which is defined as the number of moles of solute divided by the volume of the solution in liters. In this problem, the initial concentrations of Br<sub>2</sub> and Cl<sub>2</sub> must be calculated based on the given moles and the volume of the container. These initial concentrations are essential for applying the equilibrium expression and finding the equilibrium concentrations of all species involved.
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07:35Calculate Concentration of the Basic Form
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Domanda del libro di testo
At 218°C, 𝐾𝑐 = 1.2×10−4 for the equilibrium NH4SH(𝑠) ⇌ NH3(𝑔) + H2S(𝑔) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218°C and decomposes until equilibrium is reached.
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Domanda del libro di testo
At 2000°C, the equilibrium constant for the reaction 2 NO(𝑔) ⇌ N2(𝑔) + O2(𝑔) is 𝐾𝑐 = 2.4×103. If the initial concentration of NO is 0.175 M, what are the equilibrium concentrations of NO, N2, and O2?
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