Galvanic Cells 1

Given the standard reduction potentials, E^o of iron is -0.44V and E^o of oxygen is 1.23V.

what will be the emf of the cell?

• -0.79V

• -1.67V

• 1.67V

• 0.79V

Galvanic cell converts

• Chemical energy into electrical energy

• Electrical energy into chemical energy

• a metal from its elemental form to combined form

• Electrolyte into individual ions

At equilibrium

• Cell potential will be zero

• Equilibrium constant becomes equal to electrode potential

• Equilibrium constant becomes zero

• Cell potential becomes unity

For this electrochemical cell, what is the expected observation at cathode?

• Copper metal dissolves

• reddish brown solid deposited

• Silvery grey solid deposited

• Silver metal dissolves

What is the direction of electron flow.

• From Zn to Cu through the external circuit

• From Zn to Cu through salt bridge

• From Cu to Zn through the external circuit

• From Cu to Zn through salt bridge

What is an anode?

• It is the electrode where oxidation takes place.

• It is the electrode where reduction takes place.

• It is an aqueous solution containing an electrode.

• It is the salt bridge that connects half-cells.

In the above Galvanic Cell, which half cell is undergoing reduction?

• Cu | Cu²⁺

• Zn | Zn²⁺

Consider the galvanic cell reaction Zn (s) + Cu²⁺ (aq) → Cu (s) + Zn²⁺ (aq) When the cell is running spontaneously, which is the only true statement?

• The copper electrode loses mass and the zinc electrode is the cathode.

• The copper electrode gains mass and the copper electrode is the cathode.

• The zinc electrode gains mass and the zinc electrode is the anode.

• The zinc electrode loses mass and the zinc electrode is the cathode.

A certain galvanic cell has for its spontaneous cell reaction: Zn + HgO → ZnO + Hg

Which is the half-reaction occurring at the anode?

• HgO + 2 e- → Hg + O^2-

• Zn²⁺ + 2 e- → Zn

• Zn → Zn²⁺ + 2 e-

• ZnO + 2 e- → Zn

A VCE chemistry student sets up a galvanic cell using two standard half-cells with half reactions.
Half-cell 1: Cr³⁺(aq)+e^-→Cr²⁺(aq)
Half-cell 2: Cr(s)→Cr²⁺(aq)+2e^-
Sutable materials for the electrodes of te two half-cells are

• Half-cell 1: Platinum; Half-cell 2: Platinum
• Half-cell 1: Platinum; Half-cell 2: Chromium
• Half-cell 1: Chromium; Half-cell 2: Chromium
• Half-cell 1: Chromium; Half-cell 2: Platinum