The shifts of the boiling- and and freezing points in opposite directions reflects the higher energies of vapor microstates and lower energies of solid microstates in relation to those of the liquid. This reduces the temperature required to make equal numbers of states accessible in the two phases. This raises the temperature required to make equal numbers of microstates accessible in the two phases.ĭilution of the solvent adds new energy states to the liquid, but does not affect the solid phase. The red shading indicates the temperatures required to make equal numbers of microstates thermally accessible in the two phases.ĭilution of the solvent adds new energy states to the liquid, but does not affect the vapor phase. These effects are readily understood in terms of the schematic diagrams shown below. Examples such as those given below should help you connect these concepts with the real world.īoiling point elevation and freezing point depression Thermodynamics may appear at first to be a rather esoteric subject, but when you think about it, almost every chemical (and biological) process is governed by changes in entropy and free energy. What thermodynamic factors are involved in the spontaneous contraction of an elastic material such as a rubber band?. Sketch a simple electron-free energy diagram showing why a metal reacts with an oxidizing agent that is below it in the electromotive series.Sketch a simple proton-free energy diagram showing why an acid reacts with a base.Define aerobic and non-aerobic oxidation, and explain why they differ in efficiency.Describe the bioenergetic cycle of free energy in terms of the roles of glucose, electron-acceptors, ATP, and photosynthesis.Explain the critical role of temperature in the extraction of metals from their oxide ores.Under what conditions does osmotic flow occur? What is the fundamental driving force? What is the definition of osmotic pressure?.Describe the effect of increasing the hydrostatic pressure on a liquid has on its vapor pressure, and suggest a reason for this.How does the addition of a nonvolatile solute upset this balance in the two cases? At the melting and boiling points, the two phases in equilibrium have equal numbers of energetically accessible microstates.What do all of the colligative properties of solutions have in common in terms of entropy?.You are expected to be able to define and explain the significance of terms identified in bold
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