Which of the following electrodes will act as anodes, which connected to Standard Hydrogen Electrode?

Options

A. `Al//Al^(3+)" "E^(Θ) =-1.66`
B. `Fe//Fe^(2+)" "E^(Θ)=-0.44`
C. `Cu//Cu^(2+)" "E^(Θ)=+0.34`
D. `F_(2)(g)//2F^(-)(aq)" "E^(Θ)=02.87`

Explanation

To determine which electrodes will act as anodes when connected to the Standard Hydrogen Electrode (SHE), we need to analyze the given options based on their standard reduction potential values.

### Step-by-Step Solution:

1. **Understand the Standard Hydrogen Electrode (SHE):**
The SHE is defined as having a standard electrode potential of 0 volts. It serves as a reference point for measuring the electrode potentials of other half-reactions.

2. **Identify the Electrode Potentials:**
We are given the following electrodes and their standard reduction potentials:
- Aluminium (Al³⁺/Al): -1.66 V
- Iron (Fe²⁺/Fe): -0.44 V
- Copper (Cu²⁺/Cu): +0.34 V
- Fluorine (F₂/F⁻): +2.87 V

3. **Determine the Reducing Strength:**
The more negative the standard reduction potential, the stronger the reducing agent. Therefore, electrodes with negative potentials will act as anodes when connected to the SHE, as they will oxidize (lose electrons).

4. **Analyze Each Electrode:**
- **Aluminium (Al):** -1.66 V (negative potential, stronger reducing agent)
- **Iron (Fe):** -0.44 V (negative potential, stronger reducing agent)
- **Copper (Cu):** +0.34 V (positive potential, weaker reducing agent)
- **Fluorine (F):** +2.87 V (positive potential, weakest reducing agent)

5. **Conclusion:**
The electrodes that will act as anodes when connected to the SHE are Aluminium (Al) and Iron (Fe) because they have negative electrode potentials.

### Final Answer:
The electrodes that will act as anodes when connected to the Standard Hydrogen Electrode are:
- Aluminium (Al)
- Iron (Fe)