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 standard reduction potentials of the given electrodes. The electrodes with negative standard reduction potentials will act as anodes because they are stronger reducing agents than hydrogen.

### Step-by-Step Solution:

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

2. **Identify the Electrode Potentials**:
- We need to look at the standard reduction potentials of the electrodes given in the options. The reduction potentials are typically given in volts (V).
- For example:
- Aluminum (Al³⁺ + 3e⁻ → Al) has a standard reduction potential of -1.66 V.
- Iron (Fe²⁺ + 2e⁻ → Fe) has a standard reduction potential of -0.44 V.

3. **Determine the Nature of the Electrode**:
- Electrode potentials that are negative indicate that the species is a stronger reducing agent compared to hydrogen.
- Therefore, the electrodes with negative potentials will act as anodes when connected to the SHE.

4. **Analyze the Options**:
- Based on the provided reduction potentials:
- **Aluminum (Al³⁺/Al)**: -1.66 V (negative, acts as anode)
- **Iron (Fe²⁺/Fe)**: -0.44 V (negative, acts as anode)
- Other electrodes with positive potentials will not act as anodes.

5. **Conclusion**:
- The electrodes that will act as anodes when connected to the Standard Hydrogen Electrode are:
- **Option 1: Aluminum**
- **Option 2: Iron**

### Final Answer:
- The electrodes that will act as anodes when connected to the Standard Hydrogen Electrode are Aluminum and Iron.