`E^(0)` for `H^(+)//H_(2)` is

Options

A. 0
B. `+1 V`
C. `-1.0V`
D. `-2.0`V

Answer

To find the standard electrode potential \( E^{0} \) for the hydrogen electrode \( H^{+} // H_{2} \), we can follow these steps:

### Step-by-Step Solution

1. **Understanding Standard Electrode Potential**:
- The standard electrode potential (\( E^{0} \)) is a measure of the tendency of a chemical species to be reduced, and it is always measured relative to a standard reference electrode.

2. **Identifying the Reference Electrode**:
- In electrochemistry, the standard hydrogen electrode (SHE) is used as the reference electrode. This electrode consists of a platinum electrode in contact with a 1 M solution of \( H^{+} \) ions and hydrogen gas at 1 atm pressure.

3. **Defining the Value of the Standard Hydrogen Electrode**:
- The potential of the standard hydrogen electrode is defined to be zero volts (\( 0 \, V \)). This means that all other electrode potentials are measured relative to this reference point.

4. **Conclusion**:
- Therefore, the standard electrode potential \( E^{0} \) for the half-cell reaction \( H^{+} // H_{2} \) is:
\[ E^{0} = 0 \, V \]

### Final Answer
The standard electrode potential \( E^{0} \) for \( H^{+} // H_{2} \) is \( 0 \, V \).

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