Textbook Question
Write the expressions for 𝐾𝑐 for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous.
(b) Ti(𝑠) + 2Cl2(𝑔) ⇌ TiCl4(𝑙)
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Ch.15 - Chemical Equilibrium
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 15, Problem 22
Calculate Kc at 303 K for SO2(g) + Cl2(g) ⇌ SO2Cl2(g) if Kp = 34.5 at this temperature.
Verified step by step guidance1
Identify the relationship between Kc and Kp using the equation: Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
Determine Δn for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g). Calculate Δn as the difference in moles of gaseous products and reactants: Δn = moles of products - moles of reactants.
Substitute the known values into the equation: Kp = Kc(RT)^(Δn). Use R = 0.0821 L·atm/(mol·K) for the ideal gas constant and T = 303 K.
Rearrange the equation to solve for Kc: Kc = Kp / (RT)^(Δn).
Substitute the values of Kp, R, T, and Δn into the rearranged equation to find Kc.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Equilibrium Constants (Kc and Kp)
Kc and Kp are equilibrium constants that describe the ratio of concentrations or partial pressures of products to reactants at equilibrium. Kc is used for concentrations in mol/L, while Kp is used for partial pressures in atm. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas during the reaction.
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02:06
Kp vs. Kc Formula
Ideal Gas Law
The Ideal Gas Law (PV = nRT) relates the pressure, volume, temperature, and number of moles of an ideal gas. It is essential for understanding how gases behave under different conditions and is used to derive Kp from Kc. The law assumes that gas particles do not interact and occupy no volume, which is a good approximation under many conditions.
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01:15Ideal Gas Law Formula
Temperature Dependence of Equilibrium Constants
Equilibrium constants are temperature-dependent, meaning that a change in temperature can alter the values of Kc and Kp. For a given reaction, Kp and Kc can be related through the ideal gas law, but their specific values will vary with temperature. Understanding this relationship is crucial for calculating Kc from Kp when the temperature is specified.
Related Practice
Textbook Question
Consider the following equilibrium: 2 H2(g) + S2(g) ⇌ 2 H2S(g) Kc = 1.08 × 107 at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H2(g) + 1/2 S2(g) ⇌ H2S(g)
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Textbook Question
Consider the following equilibrium: 2 H2(g) + S2(g) ⇌ 2 H2S(g) Kc = 1.08 × 107 at 700°C (b) Does the equilibrium mixture contain mostly H2 and S2 or mostly H2S?