electrochemisty

Question 1

galvanic cells

Answer 1

spontaneous rxn

Question 2

electrolytic cells

Answer 2

non-spontaneous rxn

Question 3

3 types of cells

Answer 3

galvanic (voltaic), electrolytic and concentration cells

Question 4

do all cells have electrodes?

Answer 4

yes

Question 5

what’s the purpose of the electrodes

Answer 5

oxi/red rxn

Question 6

for ALL electrochemical cells (the 3 types) whats the purpose of the anode and cathode

Answer 6

AN OX (lossing e-)
RED CAT (gaining e-)

Question 7

if emf is positive

Answer 7

the cell can release energy and is spontaneous

Question 8

movement of electrons in all Electrochem cells?

Answer 8

anode to cathode

Question 9

current runs?

Answer 9

opposite electrons–> so from cathode to anode ( from the plus side!)

Question 10

what are all batteries influences by?

Answer 10

temperature changes

- bad in cold - thermodynamic issue

Question 11

flashlights have?

Answer 11

galvanic batteries

Question 12

galvanic emf and delta G

Answer 12

+, -

Question 13

galvanic cell structure

Answer 13

• 2 electrode (different) seperated in 2 compartments called half-cells, but connected with a conductive wire
• surrounding each electrode is an electrolyte solution with cations and anions (could be the same element as the metal)
• salt bridge connecting to solutions

Question 14

how do we harness energy from galvanic cells

Answer 14

separate the oxidation and reduction (which is spontaneous)but connect them by wire- so that electrons will move through wire (PE–> KE) use this energy to do work

Question 15

what happens to a zinc anode in an aqueous ZnSO4 solution?

Answer 15

anode- oxidized, so the solide Zn is oxidized (lossing e-) and becomes Zn2+

Zn–> Zn2+ + 2e-

Question 16

what happens to the Cu cathode

Answer 16

it gets the incoming 2e- coming from Zn oxidation, and the aqueous Cu2+ becomes –> Cu solid (the cathode bar)

the net reaction is

Zn + Cu2+ —> Zn2+ + Cu and E cell = +1.102 V