The potential of standard hydrogen electrode is zero. This implies that

Options

A. `DeltaG_(f)^(o)(H^(+),aq)=0`
B. `DeltaH_(f)^(o)(H^(+),aq)=0`
C. `DeltaG_(f)^(o)(H^(+),aq)lt0`
D. `DeltaG_(f)^(o)(H^(+),aq)gt0`

Explanation

To solve the question regarding the standard hydrogen electrode (SHE) and its potential being zero, we can break it down into the following steps:

### Step 1: Understanding the Standard Hydrogen Electrode
The standard hydrogen electrode (SHE) is a reference electrode used in electrochemistry. It is defined under standard conditions (1 M H⁺ concentration, 1 atm pressure of H₂ gas, and a temperature of 25°C).

### Step 2: Definition of Electrode Potential
Electrode potential is the measure of the tendency of a chemical species to be reduced, which is measured in volts (V). The SHE is assigned a potential of 0 volts by convention.

### Step 3: Implication of Zero Potential
The fact that the potential of the SHE is defined as zero implies that it serves as a baseline or reference point against which all other electrode potentials are measured.

### Step 4: Relative Measurement
When we say the potential of the SHE is zero, it indicates that any other electrode potential measured will be relative to this zero point. For example, if another electrode has a potential of +0.76 V, it means it is 0.76 V more positive than the SHE.

### Step 5: Importance in Electrochemistry
The zero potential of the SHE is crucial in determining the standard electrode potentials of other half-cells in electrochemical cells. It allows for the comparison of the reducing and oxidizing abilities of different substances.

### Conclusion
In summary, the potential of the standard hydrogen electrode being zero implies that it is the reference point for measuring all other electrode potentials in electrochemistry.

---