Chapter 18 & Chapter 19

Question 1

Define Oxidation

Answer 1

The loss of electrons

Question 2

Define Reduction

Answer 2

The gain of electrons

Question 3

Oxidation is known as the __________ in oxidation state

Answer 3

Increase

Question 4

Reduction is known as the __________ reduction state

Answer 4

Decrease

Question 5

What is the oxidation state of S in KHSO4?

Answer 5

+6

Question 6

What is the oxidation state of Carbon in CO3 2-

Answer 6

+4

Question 7

What is the oxidation states of the following? 
I) Cl2 
II) Na+ 
III) KF 
IV) CO2 
V) FeSO4

Answer 7

I) O 
II) +1 
III) K: +1, F: -1 
IV) C: +4, O: -2
V): Fe:+6, SO4: -2

Question 8

What is the oxidation states of the following? 
I) Ag 
II) Fe3+ 
III) CH4 
IV) Cr2O7 2- 
V) ClO4- 
VI) CaH2

Answer 8

I) 0 
II) +3 
III) C: -4, H: +1 
IV) Cr: +6, O: -2 
V) Cl: +7, O: -2 
VI) Ca: -2 H: +1

Question 9

Define Voltaic (Galvanic) Cell

Answer 9

Cell that PRODUCES electrical current from a SPONTANEOUS chemical reaction

Question 10

Define Electrolytic Cell

Answer 10

Cell that CONSUMES electrical current to drive a NONSPONTANEOUS chemical reaction

Question 11

Which type of cell has a system that does work on the surroundings?

Answer 11

Voltaic Cell

Question 12

Which type of cell has the desired outcome of creating electricity?

Answer 12

Voltaic Cell

Question 13

Which type of cell has a surrounding that does work on the system?

Answer 13

Electrolytic Cell

Question 14

Which type of cell has the desired outcome of creating a chemical reaction?

Answer 14

Electrolytic Cell

Question 15

What are the components that make up a Voltaic Cell?

Answer 15

2 half cells, 2 electrodes, 2 aqueous electrolyte solutions, a wire connecting the electrodes, and one salt bridge

Question 16

What are the 2 ways of writing out a cell notation?

Answer 16

I) Anode | Electrolyte || Electrolyte | Cathode | Pt

II) Fe (s) | Fe2+ (aq) || MnO4- (aq), H+, Mn2+ (aq) | Pt

Question 17

ΔGrxn < 0 = ???

Answer 17

(Q < K) Spontaneous, reaction moves to the right

Question 18

ΔGrxn > 0 = ???

Answer 18

(Q > K) Nonspontaneous, reaction moves to the left

Question 19

ΔGrxn = 0 ???

Answer 19

(Q = K) At equilibrium, reaction moves neither way

Question 20

When solving for ΔGrxn using Hess’s Law, when a chemical reaction is multiplied by a factor what happens to the ΔGrxn?

Answer 20

Also multiplied by the same factor

Question 21

When solving for ΔGrxn using Hess’s Law, when a chemical reaction is reversed what happens to the ΔGrxn?

Answer 21

It changes signs

Question 22

What is the equation used when calculating Free Energy ΔGrxn of nonstandard amounts?

Answer 22

ΔGrxn = ΔG^o rxn + RTlnQ

Question 23

What is the oxidation state of a free element?

Answer 23

0

Question 24

What is the oxidation state of H?

Answer 24

+1

Question 25

What is the oxidation state of O?

Answer 25

-2

Question 26

Define Anode

Answer 26

Electrode where Oxidation occurs

Question 27

Define Cathode

Answer 27

Electrode where Reduction occurs

Question 28

T/F Electrons flow from Cathode to Anode

Answer 28

False; electrons flow from Anode to Cathode

Question 29

What is the equation used to calculate Cell Potential?

Answer 29

E^o cell = E^o final (Cathode) - E^o initial (Anode)

Question 30

What is the equation used to calculate ΔG^o from Cell Potential?

Answer 30

ΔG^o = -nF(E^o cell)

Question 31

In the equation ΔG^o = -nF(E^o cell), what does F represent?

Answer 31

Faraday’s constant (96485)

Question 32

What is the equation used to calculate K from Cell Potential at standard conditions?

Answer 32

E^o cell = 0.0592V/n (logK)

Question 33

What is the equation used to calculate Cell Potential of nonstandard concentrations at standard conditions?

Answer 33

E cell = E^o cell - 0.0592V/n (logQ)

Question 34

If E^o cell > 0 it is…

Answer 34

Spontaneous (Voltaic Cell)

Question 35

If E^o cell < 0 it is…

Answer 35

Nonspontaneous (Electrolytic Cell)