Unit 10: Thermodynamics. Unit 10: Thermodynamics.

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Presentation transcript:

Unit 10: Thermodynamics

Entropy, S A measure of how energy is dispersed (spread out) among atoms and molecules in a system. Think DISORDER !!! Mathematical expression and units -

C (s, diamond) S = 2.38 𝑱 𝑲 𝒎𝒐𝒍 CCl4 (l) S = 214.4 𝑱 𝑲 𝒎𝒐𝒍 Entropy, S Entropy values are assigned to substances based on the third law of thermodynamics … 3rd Law of Thermo: A perfect crystalline solid at 0 Kelvin has zero entropy, S = 0. C (s, diamond) S = 2.38 𝑱 𝑲 𝒎𝒐𝒍 CCl4 (l) S = 214.4 𝑱 𝑲 𝒎𝒐𝒍 CCl4 (g) S = 309.7 𝑱 𝑲 𝒎𝒐𝒍

Entropy, S Predicting entropy changes: Entropy increases when … 1. Solids  liquids or gases 2. Liquids  gases 3. Less moles  more moles (if all states of matter are the same) 4. Solid  aqueous (dissolving) 5. Mixing or heating occurs

Entropy, S Mg (s) + O2 (g)  MgO (s) N2 (g) + 3 H2 (g)  2 NH3 (g) Is entropy increasing or decreasing in each of the following reaction? I2 (g)  I2 (l) Mg (s) + O2 (g)  MgO (s) N2 (g) + 3 H2 (g)  2 NH3 (g) What is the sign of the entropy change for each reaction?

Determining Entropy Values: The best thing about thermodynamics is that whatever works for one thermo property, works for the others!!! 2 NO (g) + O2 (g)  2 NO2 (g) Substance ∆Hf S NO 90.29 KJ/mol 210.76 J/K mol O2 0 KJ/mol 205.07 J/K mol NO2 33.1 KJ/mol 240.04 J/K mol a. Determine the ∆H for the reaction shown. Endo- or exothermic? b. Determine the ∆S for the reaction shown. What you would expect?