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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 80b
Capitolo 15, Problema 80b

For the equilibrium PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) 𝐾𝑝 = 0.052 at 60 °C. (b) After 3.00 g of solid PH3BCl3 is added to a closed 1.500-L vessel at 60 °C, the vessel is charged with 0.0500 g of BCl3(𝑔). What is the equilibrium concentration of PH3?

Guida verificata passo dopo passo
1
Convert the mass of BCl_3(g) to moles using its molar mass.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in moles of each species.
Use the initial moles of BCl_3(g) and the stoichiometry of the reaction to express the changes in moles of PH_3(g) and BCl_3(g) in terms of a variable x.
Write the expression for K_p in terms of the partial pressures of PH_3(g) and BCl_3(g), and relate these to their concentrations using the ideal gas law.
Solve the K_p expression for x, which represents the change in moles of PH_3(g), and calculate the equilibrium concentration of PH_3(g) using the volume of the vessel.

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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 scenario, the equilibrium constant (Kp) quantifies the ratio of the partial pressures of the gaseous products to that of the solid reactant, indicating the extent of the reaction at a given temperature.
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Chemical Equilibrium Concepts

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a dimensionless value that expresses the relationship between the concentrations (or partial pressures) of reactants and products at equilibrium. For the reaction PH3BCl3(s) ⇌ PH3(g) + BCl3(g), Kp = 0.052 indicates that at equilibrium, the concentration of gaseous products is relatively low compared to the solid reactant, reflecting the position of equilibrium.
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Equilibrium Constant Expressions

Stoichiometry and Concentration Calculations

Stoichiometry involves using the coefficients of a balanced chemical equation to relate the amounts of reactants and products. In this problem, the initial amounts of PH3BCl3 and BCl3 must be converted to moles, and then the changes in concentration due to the reaction must be calculated to determine the equilibrium concentration of PH3, taking into account the volume of the vessel.
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Stoichiometric Rate Calculations
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A 0.831-g sample of SO3 is placed in a 1.00-L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2SO3(𝑔) ⇌ 2 SO2(𝑔) + O2(𝑔) At equilibrium, the total pressure in the container is 1.300 atm. Find the values of 𝐾𝑝 and 𝐾𝑐 for this reaction at 1100 K.

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Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(𝑔) + Cl2(𝑔) ⇌ 2 NOCl(𝑔) At 700 K, the equilibrium constant Kp for this reaction is 0.26. Predict the behavior of each of the following mixtures at this temperature and indicate whether or not the mixtures are at equilibrium. If not, state whether the mixture will need to produce more products or reactants to reach equilibrium.

(a) PNO = 0.15 atm, PCl2 = 0.31 atm, PNOCl = 0.11 atm

(b) PNO = 0.12 atm, PCl2 = 0.10 atm, PNOCl = 0.050 atm

(c) PNO = 0.15 atm, PCl2 = 0.20 atm, PNOCl = 5.10 × 10-3 atm

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As shown in Table 15.2, the equilibrium constant for the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) is Kp = 4.34 × 10-3 at 300°C. Pure NH3 is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH3 in the equilibrium mixture. (b) What was the initial mass of ammonia placed in the vessel?

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