Why is the standard reduction potential E, for the standard hydrogen electrode 0.00V?

Please help me explain the reason why to this problem

Each electrode defines a half cell. Two half cells make up a complete electrochemical cell.

The assignment of 0.00 volts for the hydrogen electrode potential is arbitrary. It was chosen because it is easy to construct, it behaves in a consistent, reproducible manner, and it divides common electrode potentials into roughly equal numbers of positive and negative values.
The reason for assigning the reference value of zero to ONE electrode makes it possible to measure the potentials of other electrodes in a consistent way. They do that by constructing a complete electrochemical cell with two half cells, one of each is the hydrogen half cell. The voltage reading is the half cell potential of the OTHER electrode.

The standard reduction potential (E°) for the standard hydrogen electrode is defined as zero volts (0.00V). This convention is chosen as a reference point for measuring the reduction potentials of other half-reactions and helps establish a benchmark for comparison.

The standard hydrogen electrode consists of a platinum electrode immersed in a solution of 1 M hydrogen ion (H+) with a pressure of 1 bar. The half-reaction that occurs at this electrode is the reduction of hydrogen ions to hydrogen gas:

2H+ + 2e- -> H2

The standard reduction potential is determined by measuring the potential difference between the standard hydrogen electrode and another electrode of interest. By convention, the potential of the standard hydrogen electrode is set to zero volts.

This choice is made because hydrogen gas can be easily produced or consumed under standard conditions. Therefore, measurement of the potential of any other half-reaction can be compared to the potential of the standard hydrogen electrode to determine the relative oxidation or reduction tendencies.

In summary, the standard reduction potential for the standard hydrogen electrode is defined as zero volts (0.00V) to serve as a reference point for measuring reduction potentials of other half-reactions.

The standard reduction potential, E, for the standard hydrogen electrode is defined as 0.00V by convention. This is because the standard hydrogen electrode is used as a reference in electrochemical measurements and all other reduction potentials are compared to it.

To understand why the standard reduction potential for the standard hydrogen electrode is assigned as 0.00V, we need to look at its construction and the half-cell reaction it represents. The standard hydrogen electrode consists of a platinum electrode immersed in a solution of hydrogen gas at a pressure of 1 bar (or 1 atmosphere), with the hydrogen gas being bubbled through the solution.

The half-cell reaction at the standard hydrogen electrode is the reduction of hydrogen ions (H+) to hydrogen gas (H2). The balanced half-reaction equation is:

2H+ (aq) + 2e- → H2 (g)

At standard conditions (25°C, 1 bar), this half-cell reaction has a standard reduction potential of exactly 0.00V. This means that the reduction of 2 moles of H+ ions to form hydrogen gas is neither spontaneous nor non-spontaneous.

By assigning a value of 0.00V to the standard reduction potential of the standard hydrogen electrode, it allows for easy comparison and determination of the reduction potentials of other half-cell reactions. When a different half-cell reaction is connected to the standard hydrogen electrode and a potential difference is measured, we can determine whether the reaction is spontaneous (positive potential difference) or non-spontaneous (negative potential difference) relative to the reference electrode.

To summarize, the standard reduction potential of the standard hydrogen electrode is 0.00V because it serves as a reference point in electrochemical measurements, allowing for comparison of other half-cell reactions. The choice of 0.00V as the reference value simplifies the determination of the potential differences for other reactions.