Question

Standard hydrogen electrode is represented as $ Pt(s) $ , $ {H^ + }(aq)|{H_2}(g) $ .
A. True
B. False

Answer 1

Hint: In order to answer the question, first we should have explained the Standard Hydrogen Electrode and then on the basis of the definition of Standard Hydrogen Electrode, we will conclude the given representation is correct or not.

Complete step by step solution:
No, the Standard hydrogen electrode is not represented as $ Pt(s) $ , $ {H^ + }(aq)|{H_2}(g) $ .
The outside components are the electrodes for the reaction while the inner parts are the solutions they are immersed in.
Here you can see that a solid form of the reactant, Platinum, is used. The platinum, as well as the hydrogen, are participating as reactants and electrodes.
The standard hydrogen electrode (abbreviated SHE), is a redox terminal which shapes the basis of the thermodynamic size of oxidation-reduction potentials. Its total cathode potential is assessed to be $ 4.44 \pm 0.02V $ at $ {25^ \circ }C $ , anyway to shape an explanation behind assessment with any leftover terminal reactions, hydrogen's standard anode potential is articulated to be zero volts at any temperature.
Possibilities of some different terminals are looked at and that of the standard hydrogen anode at a comparative temperature. Standard hydrogen anode is a terminal that researchers use for reference on all half-cell likely responses. The assessment of the standard anode potential is zero, which outlines the reason one prerequisites to figure cell possibilities using different cathodes or different core interests.
Hydrogen electrode is based on the redox half cell: This redox reaction occurs at a platinized platinum electrode. The electrode is plunged in an acidic arrangement and unadulterated hydrogen gas is risen through it.
Hence, the correct option is (B.) False.

Note:
Standard hydrogen electrode can be used as anode half-cell or cathode half-cell depending on the requirement according to another half-cell. When a standard hydrogen electrode is attached as anode half-cell then oxidation occurs on it.