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Derive the van't Hoff equation, dIn K ΔΗ' dT RT2 which gives the dependence of the equilibrium constant on temperature.* Here AH° is the enthalpy change of the reaction, for pure substances in their standard states (1 bar pressure for gases). Notice that if AH° is positive (loosely speaking, if the reaction requires the absorption of heat), then higher temperature makes the reaction tend more to the right, as you might expect. Often you can neglect the temperature dependence of AH°; solve the equation in this case to obtain In K(T3) – In K(T) = G-) AH° 1 1 R

Derive the van't Hoff equation, dIn K ΔΗ' dT RT2 which gives the dependence of the equilibrium constant on temperature.* Here AH° is the enthalpy change of the reaction, for pure substances in their standard states (1 bar pressure for gases). Notice that if AH° is positive (loosely speaking, if the reaction requires the absorption of heat), then higher temperature makes the reaction tend more to the right, as you might expect. Often you can neglect the temperature dependence of AH°; solve the equation in this case to obtain In K(T3) – In K(T) = G-) AH° 1 1 R

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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The standard enthalpy change upon dissolving one mole of oxygen at 25°C is -11.7 kJ. Use this number and the van't Hoff equation (attached) to calculate the equilibrium (Henry's law) constant for oxygen in water at O°C and at 100°C. Discuss the results briefly.

Derive the van't Hoff equation, dIn K ΔΗ' dT RT2 which gives the dependence of the equilibrium constant on temperature.* Here AH° is the enthalpy change of the reaction, for pure substances in their standard states (1 bar pressure for gases). Notice that if AH° is positive (loosely speaking, if the reaction requires the absorption of heat), then higher temperature makes the reaction tend more to the right, as you might expect. Often you can neglect the temperature dependence of AH°; solve the equation in this case to obtain In K(T3) – In K(T) = G-) AH° 1 1 R
Transcribed Image Text:Derive the van't Hoff equation, dIn K ΔΗ' dT RT2 which gives the dependence of the equilibrium constant on temperature.* Here AH° is the enthalpy change of the reaction, for pure substances in their standard states (1 bar pressure for gases). Notice that if AH° is positive (loosely speaking, if the reaction requires the absorption of heat), then higher temperature makes the reaction tend more to the right, as you might expect. Often you can neglect the temperature dependence of AH°; solve the equation in this case to obtain In K(T3) – In K(T) = G-) AH° 1 1 R
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