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## Chem 113 Week 8

by: Caroline Hurlbut

23

0

1

# Chem 113 Week 8 Chem 113

Caroline Hurlbut
CSU
GPA 3.7

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Equilibrium and thermodynamics modified equation and example calculation
COURSE
General Chemistry II
PROF.
Ingrid Marie Laughman
TYPE
Class Notes
PAGES
1
WORDS
CONCEPTS
Chemistry
KARMA
25 ?

## Popular in Chemistry

This 1 page Class Notes was uploaded by Caroline Hurlbut on Friday March 11, 2016. The Class Notes belongs to Chem 113 at Colorado State University taught by Ingrid Marie Laughman in Spring 2016. Since its upload, it has received 23 views. For similar materials see General Chemistry II in Chemistry at Colorado State University.

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Date Created: 03/11/16
Equilibrium & Thermodynamics • ∆G = ∆Grxn + RT(lnQ) —calculate ∆Grxn —at equilibrium, 0 = ∆Grxn + RT(lnK) or ∆Grxn = -RT(lnK) • ex. N2H4(g)⁶N2(g) + 2H2(g) at 298K ∆G˚ N2H4(g) = 159.4 kJ/mol ∆G˚ N2(g) = ∆G˚H2(g) = 0.0 kJ/mol Calculate K: ∆G˚rxn = [0(1) + 0(2)] - [159.4(1)] = -159.4 kJ/mol *Calculate ∆G˚rxn K = e^[159.4 x 10^3/(8.314 x 298)] *Rearrange ∆Grxn = -RT(lnK) to K = e^(-∆Grxn/RT) and convert kJ/mol to J/mol K = 8.76 x 10^27 • another way to write the equation: lnK = (-∆H/RT) + (∆S/R) —substitute ∆Grxn for ∆H - T∆S

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