Domanda del libro di testo
At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) If the equilibrium partial pressures of NOBr(𝑔) and Br2(𝑔) are both 0.100 atm at 373 K, what is the equilibrium partial pressure of NO(𝑔)?
Ch.15 - Chemical Equilibrium
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 15, Problema 57
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
Pratica correlata
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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Domanda del libro di testo
Consider the following equilibrium, for which Δ𝐻<0
2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)
(e) the total pressure of the system is increased by adding a noble gas