Electrochemistry-1

Electrons always flow from

• cathode to anode

• anode to cathode

Tags

NGSS.HS-PS2-5

NGSS.HS-PS3-5

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

An iron nail is put into a solution of copper nitrate, iron is above copper in the activity series of metals, what will happen?

• iron will be reduced
• bubbles of oxygen gas will form on iron nail
• the iron nail will become copper plated
• no reaction occurs

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

What occurs to the mass of copper electrode in the following reaction?

Zn/Zn²⁺ // Cu²⁺/Cu

• increases

• decreases

• remains the same

Tags

NGSS.HS-PS1-7

Which metal is the negative electrode?

Zn/Zn²⁺ // Cu²⁺/Cu

• zinc

• copper

Tags

NGSS.HS-PS1-1

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 would be the theoretical cell potential of the previous electrochemical cell?

Ag⁺/Ag = 0.80V

Ni²⁺/Ni = -0.25V

• 1.05V

• -1.05V

• 0.55V

• -0.55V

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

An oxidizing agent will

• increase in mass

• lose electrons

• be reduced

• increase in oxidation number

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

In the following reaction

Sn⁺² + 2Fe⁺³ --> Sn⁺⁴ + 2Fe⁺²,

the reducing agent is...

• Fe⁺³

• Sn⁺²

• Sn⁺⁴

• Fe⁺²

Tags

NGSS.HS-PS1-2