redox II

Question 1

E°cell =

Answer 1

E°red - E°ox

Question 2

Standard conditions

Answer 2

1 mol/dm-3
298 K
100 Kpa

Question 3

If both ions are (aq)

Answer 3

use a platinum electrode

Question 4

what does a salt bridge do?

Answer 4

• closes circuit
• prevents accumulation of charge

Question 5

if E°cell is positive then what is enthalpy

Answer 5

negative (exothermic)
vice versa

Question 6

Why is Platinum used in the S.H.E electrode?

Answer 6

• porous
• unreactive

allows for easy electron transfer

Question 7

What side is the S.H.E?

Answer 7

Left side

Question 8

E°cell = +

Answer 8

feasible reaction

Question 9

ΔG (e-cell) =

Answer 9

-n*faradays constant *E°cell

Question 10

E°cell & ΔS relationship

Answer 10

directly proportional

Question 11

E°cell & Ln K

Answer 11

directly proportional

Question 12

Organic Fuel Cell Reaction

Answer 12

1) C2H5OH + 3H2O —> 2CO2 + 12H+ + 12e-
2) 3O2 + 12e- + 12H+ —-> 6H2O

Overall equation: C2H5OH + 3O2 —> 3H2O + 2CO2

Question 13

Hydrogen Fuel Cell reaction

Answer 13

1) 2H2 + 4OH- —-> 4H2O + 4e-
2) 2O2 + 4e- + 2H2O —> 4OH -

Overall: 2H2 + 2O2 –> 2H2O

Question 14

pros of a hydrogen fuel cell

Answer 14

• no greenhouse gas emissions
• high abundance
• efficient
• storage in multiple ways
• maintains voltage

Question 15

cons of a hydrogen fuel cell

Answer 15

• low life span
• hydrogen is explosive (storage)
• expensive due to electrolysis
• toxic to make cells

Question 16

Ratio of Fe2+: MnO4-

Answer 16

5:1

Question 17

Ratio of I2 : S2O3 : Cu2+

Answer 17

1:2:2