`E_(H^(+)//H_(2))^(0)=0.00V,` then `E_(D^(+)//D_(2))^(0)` at `25^(@)C` will be

Options

A. `0.00V`
B. more than zero `V`
C. less than zero `V`
D. can not be predicted

Explanation

To find the standard electrode potential \( E^{\circ}_{(D^{+}//D_{2})} \) at 25°C given that \( E^{\circ}_{(H^{+}//H_{2})} = 0.00 \, \text{V} \), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Standard Electrode Potential**:
The standard electrode potential \( E^{\circ} \) is a measure of the tendency of a chemical species to be reduced, and it is measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C).

2. **Comparing Hydrogen and Deuterium**:
We know that deuterium (D) is an isotope of hydrogen (H) and has similar chemical properties. However, the standard electrode potential for deuterium will differ slightly from that of hydrogen due to the differences in mass and bond energies.

3. **Using the Electrochemical Series**:
In the electrochemical series, hydrogen is assigned a standard electrode potential of 0.00 V. Since deuterium is heavier, it is expected to have a slightly lower standard reduction potential than hydrogen.

4. **Estimation of \( E^{\circ}_{(D^{+}//D_{2})} \)**:
According to the electrochemical series, the standard reduction potential for deuterium is slightly less positive than that of hydrogen. It is generally accepted that:
\[ E^{\circ}_{(D^{+}//D_{2})} \approx -0.01 \, \text{V} \]
This indicates that deuterium is less favorable for reduction compared to hydrogen.

5. **Conclusion**:
Therefore, the standard electrode potential for the deuterium half-cell at 25°C is:
\[ E^{\circ}_{(D^{+}//D_{2})} \approx -0.01 \, \text{V} \]

### Final Answer:
\[ E^{\circ}_{(D^{+}//D_{2})} \approx -0.01 \, \text{V} \]

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