In a Daniel cell, what is the direction of flow of electrons?

From Zinc to Copper electrode

In a Daniel cell, the direction of flow of electrons is from the zinc electrode to the copper electrode. Let's understand why this is the case:

The Daniel cell is a type of electrochemical cell that consists of two half-cells connected by a salt bridge or a porous barrier. One half-cell contains a zinc electrode (anode), and the other half-cell contains a copper electrode (cathode).

During the operation of the Daniel cell, a redox reaction takes place in each half-cell:

At the zinc electrode (anode):
\[ \text{Zn(s)} \rightarrow \text{Zn}^{2+}(\text{aq}) + 2\text{e}^- \]

The released electrons flow through the external circuit from the zinc electrode to the copper electrode.

At the copper electrode (cathode):
\[ \text{Cu}^{2+}(\text{aq}) + 2\text{e}^- \rightarrow \text{Cu(s)} \]

The overall cell reaction can be represented as:
\[ \text{Zn(s)} + \text{Cu}^{2+}(\text{aq}) \rightarrow \text{Zn}^{2+}(\text{aq}) + \text{Cu(s)} \]

The flow of electrons through the external circuit, from the zinc electrode (anode) to the copper electrode (cathode), creates an electric current and constitutes the production of electricity in the Daniel cell.

Therefore, the correct answer is option 2: From Zinc to Copper electrode.