Lesson_22

# Lesson_22 - Galvanic cells Cu(s Cu2(aq 2 eAg(aq e Ag(s Cu(s...

This preview shows pages 1–9. Sign up to view the full content.

Lesson 22 Galvanic cells

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Lesson 22 Definitions Oxidation takes place at the anode . Since electrons flow from the anode, it shows negative charge . Reduction takes place at the cathode . Since electrons flow to the cathode, it shows positive charge .
Lesson 22 Dry cell

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Lesson 22 Car battery
Lesson 22 Ag/Zn button battery

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Lesson 22 Hydrogen fuel cell O 2 ( g ) + 2 H 2 O( l ) + 4 e - = 4 OH - ( aq ) 2 H 2 ( g ) + 4 OH - ( aq ) = 4 H 2 O( l ) + 4 e - 2 H 2 ( g ) + O 2 ( g ) = 2 H 2 O( l )
Lesson 22 Faraday’s law “The mass of a given substance that is produced or consumed at an electrode is proportional to the quantity of electric charge passed through the cell.”

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Lesson 22 Useful definitions and relations Charge of a single electron: e = 1.6021773 x 10 -19 C (coulombs) Charge of one mole of electrons ( Faraday constant ): F = (6.022137 x 10 23 mol -1 ) (1.6021773 x 10 -19 C) = = 96,485.31 C mol -1 Electric current ( I ) is the amount of charge ( Q ) flowing through a circuit per unit of time (
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

### Page1 / 13

Lesson_22 - Galvanic cells Cu(s Cu2(aq 2 eAg(aq e Ag(s Cu(s...

This preview shows document pages 1 - 9. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online