Presentation is loading. Please wait.

Presentation is loading. Please wait.

Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg. 862-865 # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg. 862-865.

Similar presentations


Presentation on theme: "Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg. 862-865 # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg. 862-865."— Presentation transcript:

1 Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg # 40, 44, 50, 54, 60, 65, 74 - Due Fri. Apr 23

2 Workbook Lesson pkt Lesson 13 - Formal Oxidation number assignments - with examples and homework Lesson 28 - Balancing Redox Reactions with examples and homework

3 Sect (slides provided)

4 Galvanic Cell schematic Oxidation occurs at anode (vowels) Reduction occurs at cathode (consonants) Oxidation produces electrons, so current flows from anode to cathode.

5 Types of cells Standard Hydrogen cell platinum electrode metal electrodes

6 Cell Potential & Nernst Equation Galvanic Cell Potentials - free energy G o = -nFE o F is Faraday constant C/mol e- n = moles of e- from balanced Redox eqn Concentration Cell Potentials G = G o + RTlnQ or K if E cell = 0

7 Cell Potential & Nernst Equation G = G o + RT ln Q -nFE = -nFE o +RT ln Q E = E o - RT/nF ln Q E = E o /n log Q So E of a cell with concentrations not equal to 1 M is the std cell potential with the correction remember to know electrons transferred in Redox

8 Equilibrium, K constant E = E o - RT/nF log Q At equilibrium E cell = 0 and Q = K 0 = E o /n log K log K = nE o /

9 K example Example pg 841

10 Battery - Dry Cell

11

12


Download ppt "Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg. 862-865 # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg. 862-865."

Similar presentations


Ads by Google