Electrochemistry

Electrons always flow from

• cathode to anode

• anode to cathode

Oxidation occurs at the

• anode

• cathode

Electrons are gained at the

• anode

• cathode

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 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

If Al is above Co in the activity series of metals, which of the following will occur if Al metal is put into a solution of cobalt nitrate?

• a redox reaction takes place
• the Al strip dissolves
• the Al strip becomes coated with cobalt
• all of the above

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

Zn/Zn²⁺ // Cu²⁺/Cu

• increases

• decreases

• remains the same

Which metal is the negative electrode?

Zn/Zn²⁺ // Cu²⁺/Cu

• zinc

• copper

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^-

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