Electrochemistry_I

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu²⁺/Cu = 0.34V

Zn²⁺/Zn = -0.76V

• Cu

• Zn

• CuSO₄

• ZnSO₄

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-4

What reaction occurs at the anode?

Ag⁺/Ag = 0.80V

Ni²⁺/Ni = -0.25V

• Ag⁺ + e^- →Ag

• Ag → Ag⁺ + e^-

• Ni²⁺ + 2e^- → Ni

• Ni → Ni²⁺ + 2e^-

Tags

NGSS.HS-PS1-2

What is a reducing agent?

• It is the species that gets reduced -- gains electrons.

• It is the species that gets oxidized -- loses electrons.

• It is the species that creates electrons.

• It is the species that destroys electrons.

In the following reaction

Sn⁺² + 2Fe⁺³ → Sn⁺⁴ + 2Fe⁺²

the oxidizing agent is....

• Sn⁺⁴

• Sn⁺²

• Fe⁺³

• Fe⁺²

Tags

NGSS.HS-PS1-2

Which direction do the electrons flow in wire X and which metal is oxidized?

• A
• B
• C
• D

Tags

NGSS.HS-PS2-5

Galvanic cells convert

• mechanical energy in to electrical energy

• potential energy in to electrical energy

• electrical energy in to chemical energy

• chemical energy in to electrical energy

Tags

NGSS.HS-PS1-4

Consider this cell.

Select all true statements

• Zinc is a more reactive metal than copper

• Cu²⁺ is a stronger oxidising agent that Zn²⁺

• The cell potential is the sum of the two electrode potentials

• The copper electrode will get bigger as current flows

• The zinc electrode will get smaller as current flows

Answer explanation

The cell potential is the difference between electrode potentials

Copper metal will be formed from copper ions, while zinc metal will be oxidised into zinc ions.

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-4

• 5, 2, 2, 5

• 5, 2, 5, 2

• 2, 5, 2, 5

• 2, 5, 5, 2

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Calculate the cell potential of voltaic cell

• –1.51
• - 0.03
• +0.03
• +1.51

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

NGSS.HS-PS3-5

Calculate the cell potential of voltaic cell

• –1.60 V
• +1.60 V
• –3.12 V
• +3.12 V

Tags

NGSS.HS-PS3-1