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Question
Which cell will measure standard electrode potential of copper electrode?
Options
\[\ce{Pt(s) | H2 (g,0.1 bar) | H+ (aq; 1 M) || Cu^{2+} (aq;1M) | Cu}\]
\[\ce{Pt(s) | H2 (g, 1 bar) | H+ (aq; 1 M) || Cu^{2+} (aq; 2 M) | Cu}\]
\[\ce{Pt(s) | H2 (g, 1 bar) | H+ (aq; 1 M) || Cu^{2+} (aq; 1 M) | Cu}\]
\[\ce{Pt(s) | H2 (g, 1 bar) | H+ (aq; 0.1 M) || Cu^{2+} (aq; 1 M) | Cu}\]
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Solution
\[\ce{Pt(s) | H2 (g, 1 bar) | H+ (aq; 1 M) || Cu^{2+} (aq; 1 M) | Cu}\]
Explanation:
When copper electrode is connected to standard hydrogen electrode, it acts as cathode and its standard electrode potential can be measured.
`"E"^0 = "E"_"R"^0 - "E"_"L"^0 = "E"_"R"^0 - 0 = "E"_"R"^0`
To calculate the standard electrode potential of the given cell it is coupled with the standard hydrogen electrode in which pressure of hydrogen gas is one bar and the cone, of H+ ion in the solution is one molar and also the concentrations of the oxidized and the reduced forms of the species in the right-hand half-cell are unity.
