Question

In the overall electrochemical reaction:

A. nitrogen is oxidized at the anode, and hydrogen is reduced at the cathode.
B. nitrogen is reduced at the cathode, and hydrogen is oxidized at the anode.
C. nitrogen is reduced at the anode, and hydrogen is oxidized at the cathode.
D. nitrogen is oxidized at the cathode, and hydrogen is reduced at the anode.

Answer 1

Option B is correct: nitrogen is reduced at the cathode and hydrogen is oxidized at the anode in the described electrochemical reaction with the tin electrode as the anode and platinum electrode as the cathode.

Step-by-step explanation:

The answer to the question regarding the overall electrochemical reaction is that nitrogen is reduced at the cathode, and hydrogen is oxidized at the anode. This corresponds to option B: nitrogen is reduced at the cathode, and hydrogen is oxidized at the anode. In electrochemical cells, the anode is where oxidation occurs, meaning it is where electrons are lost. The cathode is the site of reduction, where electrons are gained.

The tin electrode is the anode since Sn is oxidized to Sn²+ while nitrate is reduced to NO at the platinum electrode, which acts as the cathode. Remember, in a galvanic or voltaic cell, the anode is negative and the cathode is positive, allowing electrons to flow through an external circuit from anode to cathode.