Skip to main content
Ch.19 - Free Energy & Thermodynamics
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.19 - Free Energy & ThermodynamicsProblema 82
Capitolo 19, Problema 82

Estimate the value of the equilibrium constant at 655 K for each reaction in Problem 74. (ΔHf° for BrCl is 14.6 kJ/mol.)

Guida verificata passo dopo passo
1
Identify the reaction for which you need to estimate the equilibrium constant. Since the problem refers to Problem 74, ensure you have the correct chemical equation.
Use the van 't Hoff equation to relate the change in the equilibrium constant with temperature: \( \ln \left( \frac{K_2}{K_1} \right) = -\frac{\Delta H^\circ}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right) \).
Determine the values needed for the van 't Hoff equation: \( \Delta H^\circ = 14.6 \text{ kJ/mol} \) (convert to J/mol), \( R = 8.314 \text{ J/mol K} \), and the temperatures \( T_1 \) and \( T_2 \) in Kelvin.
Assume or find the initial equilibrium constant \( K_1 \) at a known temperature \( T_1 \). If not given, you may need to use standard conditions or additional data from Problem 74.
Solve the van 't Hoff equation for \( K_2 \), the equilibrium constant at 655 K, using the values obtained in the previous steps.

Concetti chiave

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

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction at a specific temperature. It provides insight into the extent of a reaction; a large K indicates a reaction that favors products, while a small K suggests a preference for reactants.
Video consigliato:
Percorso guidato
01:14
Equilibrium Constant K

Van 't Hoff Equation

The Van 't Hoff equation relates the change in the equilibrium constant (K) with temperature to the enthalpy change (ΔH) of the reaction. It is expressed as ln(K2/K1) = -ΔH/R(1/T2 - 1/T1), where R is the gas constant. This equation is essential for estimating K at different temperatures, particularly when ΔH is known.
Video consigliato:
Percorso guidato
01:40
Van der Waals Equation

Standard Enthalpy of Formation (ΔHf°)

The standard enthalpy of formation (ΔHf°) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. It is a crucial value for calculating the overall enthalpy change of a reaction, which can then be used to determine the equilibrium constant using thermodynamic principles.
Video consigliato:
Percorso guidato
02:34
Enthalpy of Formation
Pratica correlata
Domanda del libro di testo

Determine the sign of ΔSsys for each process. a. water boiling

1191
views
Domanda del libro di testo

Consider the reaction: I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 at 25 °C Calculate ΔGrxn for the reaction at 25 °C under each of the following conditions: b. at equilibrium

977
views
Domanda del libro di testo

Consider the reaction: 2 NO(g) + O2(g) ⇌ 2 NO2(g) The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°rxn and ΔS°rxn for the reaction.

1156
views
1
comments
Domanda del libro di testo

A reaction has an equilibrium constant of 8.5⨉103 at 298 K. At 755 K, the equilibrium constant is 55.2. Find ΔH°rxn for the reaction.

Domanda del libro di testo

Consider the reaction: I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 at 25 °C Calculate ΔGrxn for the reaction at 25 °C under each of the following conditions: c. PICl = 2.55 atm; PI2 = 0.325 atm; PCl2 = 0.221 atm

2862
views