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CHEM 1310 (11)
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CHEM 1310 - Notes 6.docx

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Department
Chemistry
Course
CHEM 1310
Professor
Sarrah Vakili
Semester
Summer

Description
 ∆G reaction = products - reactants  ∆S - what can you conclude about the sign and magnitude?  ∆G = H - T S o ∆ H = 34.5 o ∆T = 450 o ∆G = -1 o -1 = 34.5 kJ -450 S o - 35500 = -450 S o ∆S = 78.9 Q.Calculate standard reaction entropy at 298 K for: o 2CH3CHO + O2 → 2CH3COOH A. Sᵒ = 159.8(2) - 263.8(2) - 205.2 Gibb's Free Energy  Is a state function (constant)  Gives the amount of useable energy in the universe  May be calculated using G = H - T S  ∆G < 0 means reaction is spontaneous  The value for a reaction may be manipulated using the same methods as H and S ∆Hᵒ and Temperature  Clausius-Clapeyron often used to relate Hᵒ and Sᵒ to temperature and pressure  Is the equation of a straight line graph on lnP(y-axis) vs. 1/T(x-axis with m=slope= Hᵒ/R and b= Sᵒ/R  There are several ways to rearrange this equation mathematically and it is closely related to the van't Hoff and the Arrhenius equations o ( ) o M = o X = o B = Q.What is the pressure of H2O vapor @ 64 ᵒC, if the pressure is 22.4 mmHg @ 23 ᵒC and the molar enthalpy is 44 kJ/mol A.  ∆H = 44 kJ/mol  Constant = 8
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