Consider a salt bridge voltaic cell represented by the...

Consider a salt bridge voltaic cell represented by the following reaction: $$ \mathrm{Fe}(s)+2 \mathrm{Tl}^{+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+2 \mathrm{Tl}(s) $$ Choose the best answer from the choices in each part below: (a) What is the path of electron flow? Through the salt bridge, or through the external circuit? (b) To which half-cell do the negative ions in the salt bridge move? The anode, or the cathode? (c) Which metal is the electrode in the anode?

Consider a salt bridge voltaic cell represented by the following reaction:
$$
\mathrm{Fe}(s)+2 \mathrm{Tl}^{+}(a q) \longrightarrow \mathrm{Fe}^{2+}(a q)+2 \mathrm{Tl}(s)
$$
Choose the best answer from the choices in each part below:
(a) What is the path of electron flow? Through the salt bridge, or through the external circuit?
(b) To which half-cell do the negative ions in the salt bridge move? The anode, or the cathode?
(c) Which metal is the electrode in the anode?

Key Concepts

Voltaic Cell

A voltaic cell is an electrochemical cell that derives electrical energy from a spontaneous redox reaction occurring within the cell. In such cells, two half-cells are connected by an external circuit and an internal salt bridge, facilitating the complete circuit required for current flow.

Electron Flow and External Circuit

In a voltaic cell, electrons produced by oxidation at the anode travel through the external circuit to the cathode, where they drive the reduction reaction. The external circuit is the designated path for electron flow; electrons do not travel through the salt bridge.

Salt Bridge Function and Ion Migration

The salt bridge contains ions that migrate between the two half-cells to maintain electrical neutrality as the redox reaction proceeds. Negative ions in the salt bridge typically move toward the anode, where oxidation generates excess positive charge, while positive ions migrate toward the cathode to balance the accumulating negative charge.

Anode and Cathode Roles

The anode is the electrode where oxidation occurs—electrons are lost from the species present at this electrode—making it negatively charged. Conversely, the cathode is where reduction takes place, with electrons being gained. Identification of these roles is crucial to determining which electrode undergoes oxidation or reduction in any electrochemical cell.

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