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A standard hydrogen electrode has zero electrode potential because
- a)Hydrogen is the lightest element
- b)Hydrogen atom has only one electron.
- c)Hydrogen is easiest to oxidize
- d)The electrode potential is assumed to be zero
Correct answer is option 'D'. Can you explain this answer?
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A standard hydrogen electrode has zero electrode potential becausea)Hy...
This electrode potential is assumed to be zero
The standard potential of hydrogen electrode is assumed to be zero at all temperature.
The Standard hydrogen electrode (abbreviated SHE), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials. Its absolute electrode potential is estimated to be 4.44 � 0.02 V at 25 �C, but to form a basis for comparison with all other electrode reactions, hydrogen's standard electrode potential (E0) is declared to be zero volts at all temperatures.
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A standard hydrogen electrode has zero electrode potential becausea)Hy...
Explanation:
A standard hydrogen electrode (SHE) is an electrode that is used as a reference in half-cell reactions to determine the electrode potential of other electrodes. It consists of a platinum electrode immersed in a solution of an acid, typically 1 M HCl, with hydrogen gas bubbling through it.
The electrode potential of a standard hydrogen electrode is considered to be zero because it is used as a reference point to measure the electrode potential of other electrodes. By convention, the electrode potential of the SHE is set to zero, and all other electrode potentials are measured relative to it.
The reasons why the electrode potential of the standard hydrogen electrode is assumed to be zero are as follows:
1. Consistency and ease of measurement: By establishing the electrode potential of the SHE as zero, it provides a consistent reference point for comparing the electrode potentials of other electrodes. This makes it easier to measure and compare the electrode potentials of different reactions.
2. Hydrogen as a neutral element: Hydrogen gas (H2) is composed of two hydrogen atoms, each with one electron. These electrons can easily be lost or gained, making hydrogen a versatile element for redox reactions. Since hydrogen is a neutral element, it is considered to have an electrode potential of zero.
3. Reversibility of the hydrogen electrode: The hydrogen electrode is reversible, meaning that it can be easily converted between an oxidation half-reaction and a reduction half-reaction. This reversibility allows for accurate and reproducible measurements of electrode potentials.
4. Standardization: The choice of the standard hydrogen electrode as the reference electrode is based on convention and standardization. It provides a consistent and universally accepted reference point for measuring and comparing electrode potentials.
Overall, the assumption of a zero electrode potential for the standard hydrogen electrode simplifies the measurement and comparison of electrode potentials in electrochemical reactions. It provides a consistent reference point and allows for the standardization of electrode potential measurements.
A standard hydrogen electrode (SHE) is an electrode that is used as a reference in half-cell reactions to determine the electrode potential of other electrodes. It consists of a platinum electrode immersed in a solution of an acid, typically 1 M HCl, with hydrogen gas bubbling through it.
The electrode potential of a standard hydrogen electrode is considered to be zero because it is used as a reference point to measure the electrode potential of other electrodes. By convention, the electrode potential of the SHE is set to zero, and all other electrode potentials are measured relative to it.
The reasons why the electrode potential of the standard hydrogen electrode is assumed to be zero are as follows:
1. Consistency and ease of measurement: By establishing the electrode potential of the SHE as zero, it provides a consistent reference point for comparing the electrode potentials of other electrodes. This makes it easier to measure and compare the electrode potentials of different reactions.
2. Hydrogen as a neutral element: Hydrogen gas (H2) is composed of two hydrogen atoms, each with one electron. These electrons can easily be lost or gained, making hydrogen a versatile element for redox reactions. Since hydrogen is a neutral element, it is considered to have an electrode potential of zero.
3. Reversibility of the hydrogen electrode: The hydrogen electrode is reversible, meaning that it can be easily converted between an oxidation half-reaction and a reduction half-reaction. This reversibility allows for accurate and reproducible measurements of electrode potentials.
4. Standardization: The choice of the standard hydrogen electrode as the reference electrode is based on convention and standardization. It provides a consistent and universally accepted reference point for measuring and comparing electrode potentials.
Overall, the assumption of a zero electrode potential for the standard hydrogen electrode simplifies the measurement and comparison of electrode potentials in electrochemical reactions. It provides a consistent reference point and allows for the standardization of electrode potential measurements.
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A standard hydrogen electrode has zero electrode potential becausea)Hydrogen is the lightest elementb)Hydrogen atom has only one electron.c)Hydrogen is easiest to oxidized)The electrode potential is assumed to be zeroCorrect answer is option 'D'. Can you explain this answer?
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