# CHEM 1050 Study Guide - Final Guide: Electrochemistry, University Of Houston, Thermodynamics

by OC66277

School

University of GuelphDepartment

ChemistryCourse Code

CHEM 1050Professor

Dennis BakerStudy Guide

FinalThis

**preview**shows half of the first page. to view the full**1 pages of the document.**Equation List Chem 1050 Exam

Thermodynamics

q = mC ΔT

w = -P ΔV = - ΔnRT

ΔU = q(system) + w(system)

ΔU = ΔH - ΔnRT

ΔS = ΔH/T

ΔG° = ΔH - TΔS

ΔG° = -RTlnk(eq)

ΔG = ΔG° +RTlnQ

ΔG = RTln(Q/k)

Bomb Calorimeter (constant volume)

ΔH = ΔU + ΔnRT

ΔU = q

Coffee Cup Calorimeter (constant pressure)

ΔU = q +w

ΔH = q

Electrochemistry

ΔG° = -nFE°

ΔG° = -RTlnk(eq)

ΔG = RTln(Q/k)

E° = (RT/nF)lnk(eq)

E = E° - (RT/nF)lnQ

E = (-RT/nF) ln([anode]/[cathode])

E = cathode - anode

Q = [products]/[reactants]

Charge = It

m = MIt/Fn

*Volts is in J/C

Kinetics

Order

Rate Law

Integrated Rate Law

Straight Line Plot

(slope = -k)

Half-Life

Units

0

= k

[A]t = -kt + [A]0

[A] vs t

=[A]0/2k

1

= k[A]

ln ([A]t / [A]0) = -kt

ln[A] vs t

=ln(2)/k

s-1

2

= k[A]2

1/[A]t = kt + 1/[A]0

1/[A]t vs t

=1/k[A]0

M-1LS-1

Arrhenius

k = Ae-Ea/RT

Straight line plot = ln k vs 1/t

Slope = -Ea/R

For 2 Temperatures

ln (k2/k1) = (Ea/R)(ΔT/T2*T1)

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