Consider the electrochemical cell:

Question

Volts
1.0 M KNO3
Ag Fe
1.0 M Ag NO3 1.0 M Fe (NO3)2
a) Towards which half-cell do the NO3
−
( ) aq in the salt bridge initially move? and explain why its the Fe electrode. also explain how Fe is the anode and Ag is the cathode

Answer 1

In this electrochemical cell, the NO3- ions in the salt bridge will initially move towards the Fe electrode. This is because Fe(NO3)2 is present in higher concentration in the Fe half-cell compared to AgNO3 in the Ag half-cell.

Now, let's discuss why Fe is the anode and Ag is the cathode. In a galvanic cell, the anode is the electrode where oxidation occurs, and the cathode is the electrode where reduction occurs.

At the Fe electrode:

Fe -> Fe2+ + 2e-
This half-reaction represents the oxidation of Fe, where Fe loses electrons and gets converted into Fe2+. Therefore, Fe is undergoing oxidation and is acting as the anode.

At the Ag electrode:

Ag+ + e- -> Ag
This half-reaction represents the reduction of Ag+ ions, where Ag+ ions gain an electron and get converted into Ag. Therefore, Ag is undergoing reduction and is acting as the cathode.

Overall, in this electrochemical cell, Fe is the anode because it undergoes oxidation, and Ag is the cathode because it undergoes reduction.