Electrochemistry

Question 1

Redox reactions involves the movement of _________ from one substance to another

Answer 1

Electrons

Question 2

Oxidation is the _______ of electrons

Answer 2

Loss

Question 3

Reductions is the _______ of electrons

Answer 3

Gain

Question 4

A voltaic Cell (Galvanic Cell)

Answer 4

Uses a spontaneous redox reaction (ΔG < 0) to generate electrical energu where the system does work on the surroundings

Question 5

An electrolytic Cell

Answer 5

Uses Electrical energy to drive a nonspontaneous redox reaction (ΔG > 0) where the surroundings do work on the system

Question 6

What are the two types of electrode?

Answer 6

1. Anode
2. Cathode

Question 7

What type of half reactions occurs at the anode?

Answer 7

The oxidatio, the anode has a negative charge

Question 8

What type of reaction occurs at the Cathode?

Answer 8

Reduction, the cathode has a positive charge

Question 9

What direction does electron flow between the two electrode?

Answer 9

Flow from left ot right ( from the anode to the cathode)

Question 10

Cell potential (E_cell)

Answer 10

Is the difference in electrical potiental between the two electrode (or the two half reaction)

Question 11

Electrons flow spontaneously from the _______ to _______

Answer 11

From the anode to cathode

Question 12

The cell potential is ________ for a reaction to be spontaneous

Answer 12

Positive (E_cell > 0)

Question 13

For a nonspontaneous reaction the cell potential is _________

Answer 13

Negative (E_cell < 0)

Question 14

When the cell potential is __________ the reaction is at equilibrium

Answer 14

Equal to zero

Question 15

The standard cell potential (E^o_cell)

Answer 15

Is the sum of the sum of the electrical potential of the half reaction

Question 16

Standard cell potential are only used for a __________ reaction

Answer 16

Reduction reaction so if its an oxidation reaction just flip the sign

Question 17

What the formula for calculating the E^o_cell

Answer 17

E^o_cell = E^o_reduction - E^o_oxidation

Question 18

A strong oxidizing agent forms a ________ reducing agent & vice versa

Answer 18

Weak

Question 19

Equation used to relate ΔG^o & E^o_cell

Answer 19

ΔG^o = -nFE^o_cell

Question 20

Equation used for E^o_cell when not using standard concentration (1M)

Answer 20

E_cell = E^o_cell - 0.0592V / n log Q

Question 21

What the equation used when E^o_cell is at equilibrium and using standard condition such as 1M (& 298.15K)

Answer 21

E^o_cell = 0.0592 V/ n log K

or

log K = nE^o_cell / 0.0592V