Skip to main content
Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.15 - Chemical EquilibriumProblema 82
Capitolo 15, Problema 82

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.

Guida verificata passo dopo passo
1
Calculate the initial moles of SO3 using its molar mass. Use the formula: moles = mass (g) / molar mass (g/mol).
Set up an ICE table (Initial, Change, Equilibrium) for the reaction: 2SO3(g) ⇌ 2SO2(g) + O2(g). Assume x moles of SO3 decompose, then 2x moles of SO2 and x moles of O2 are formed.
Calculate the equilibrium partial pressures of SO3, SO2, and O2 using the ideal gas law (PV = nRT), where P is the partial pressure, n is the number of moles at equilibrium, R is the gas constant, and T is the temperature in Kelvin.
Use the equilibrium partial pressures to find the equilibrium constant Kp for the reaction. Apply the formula for Kp: Kp = (PSO2)2 * PO2 / (PSO3)2.
Convert Kp to Kc using the relationship Kc = Kp / (RT)Δn, where Δn is the change in moles of gas (products minus reactants) and T is the temperature in Kelvin.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
13m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Equilibrium Constant (Kp and Kc)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kp is used when dealing with partial pressures of gases, while Kc is used for concentrations in molarity. For the reaction 2SO3(g) ⇌ 2SO2(g) + O2(g), Kp can be calculated using the expression Kp = (P_SO2^2 * P_O2) / (P_SO3^2), where P represents the partial pressures of the gases involved.
Video consigliato:
Percorso guidato
02:06
Kp vs. Kc Formula

Decomposition Reaction

A decomposition reaction is a type of chemical reaction where a single compound breaks down into two or more simpler products. In this case, sulfur trioxide (SO3) decomposes into sulfur dioxide (SO2) and oxygen (O2). Understanding the stoichiometry of the reaction is crucial for calculating the equilibrium concentrations and subsequently the equilibrium constants.
Video consigliato:
Percorso guidato
01:30
Alcohol Reactions: Dehydration Reactions

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates the pressure (P), volume (V), number of moles (n), the ideal gas constant (R), and temperature (T) of a gas. In this problem, the total pressure at equilibrium and the volume of the container are used to determine the number of moles of each gas present. This information is essential for calculating the equilibrium concentrations needed to find Kc.
Video consigliato:
Percorso guidato
01:15
Ideal Gas Law Formula
Pratica correlata
Domanda del libro di testo

For the equilibrium PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) 𝐾𝑝 = 0.052 at 60°C. (b) A closed 1.500-L vessel at 60°C is charged with 0.0500 g of BCl3(𝑔); 3.00 g of solid PH3BCl3 is then added to the flask, and the system is allowed to equilibrate. What is the equilibrium concentration of PH3?

Domanda del libro di testo

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. For each of the following mixtures at this temperature, indicate whether the mixture is at equilibrium, or, if not, whether it needs to produce more products or reactants to reach equilibrium. (b) 𝑃NO = 0.12atm, 𝑃Cl2 = 0.10atm, 𝑃NOCl = 0.050atm

Domanda del libro di testo

At 900 °C, 𝐾𝑐 = 0.0108 for the reaction

CaCO3(𝑠) ⇌ CaO(𝑠) + CO2(𝑔)

A mixture of CaCO3, CaO, and CO2 is placed in a 10.0-L vessel at 900°C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium?

(a) 15.0 g CaCO3, 15.0 g CaO, and 4.25 g CO2

(b) 2.50 g CaCO3, 25.0 g CaO, and 5.66 g CO2

(c) 30.5 g CaCO3, 25.5 g CaO, and 6.48 g CO2

724
views
1
rank