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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.15 - Chemical EquilibriumProblema 86
Capitolo 15, Problema 86

A reaction vessel at 27 °C contains a mixture of SO2 (P = 3.00 atm) and O2 (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO2( g) + O2( g) ⇌ 2 SO3( g). At equilibrium, the total pressure is 3.75 atm. Find the value of Kc.

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1
Convert the initial temperature from Celsius to Kelvin by using the formula T(K) = T(°C) + 273.15. This will be used in later calculations involving the ideal gas law and equilibrium constants.
Calculate the initial moles of SO2 and O2 using the ideal gas law, PV = nRT, where P is the pressure of the gas, V is the volume, R is the gas constant, and T is the temperature in Kelvin.
Set up an ICE table (Initial, Change, Equilibrium) for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g). Use the initial pressures as proxies for initial concentrations, and express changes in terms of x, where x is the change in moles of O2 reacting.
Write the expression for the equilibrium constant Kp in terms of the partial pressures of the gases at equilibrium. Use the relationship between Kp and Kc, which is Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas (products minus reactants).
Solve for Kc using the equilibrium pressures calculated from the ICE table and the relationship between Kp and Kc. Substitute the values of R, T, and Δn to find Kc.

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Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. A larger Kc indicates a greater concentration of products at equilibrium, while a smaller Kc suggests a higher concentration of reactants.
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Equilibrium Constant Expressions

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In this reaction, the partial pressures of SO2 and O2 before the reaction are crucial for determining the changes in pressure as the reaction proceeds to equilibrium.
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Partial Pressure Calculation

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. In this context, adding a catalyst does not change the position of equilibrium but allows the system to reach equilibrium faster, which is important for calculating Kc based on the final pressures of the gases involved.
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Le Chatelier's Principle
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Carbon monoxide and chlorine gas react to form phosgene: CO(g) + Cl2(g) ⇌ COCl2(g) Kp = 3.10 at 700 K If a reaction mixture initially contains 215 torr of CO and 245 torr of Cl2, what is the mole fraction of COCl2 when equilibrium is reached?

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At 70 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.0 atm at equilibrium.

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The equilibrium constant for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) is Kc = 3.0. Find the amount of NO2 that must be added to 2.4 mol of SO2 in order to form 1.2 mol of SO3 at equilibrium.

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