Questions in electrochemistry

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The standard reduction potentials of 4 elements are given below. Which of the following will be the most suitable reducing agent $I = – 3.04 V$, $II = – 1.90 V$, $III = 0 V$, $IV = 1.90 V$
Standard reduction potentials at ${{25}^{o}}C$ of $L{{i}^{+}}|Li,\,B{{a}^{2+}}|Ba,\,N{{a}^{+}}|Na$ and $M{{g}^{2+}}|Mg$ are – 3.05, – 2.90, – 2.71 and – 2.37 volt respectively. Which one of the following is the strongest oxidising agent
If the standard electrode potential of $C{{u}^{2+}}/Cu$ electrode is $0.34 V$, what is the electrode potential of $0.01 M$ concentration of $C{{u}^{2+}}$ (T= 298K)
The emf of a Daniel cell at 298 K is ${{E}_{1}}Zn|\underset{(0.01\,M)}{\mathop{ZnS{{O}_{4}}}}\,||\underset{(1.0\,M)}{\mathop{CuS{{O}_{4}}}}\,|Cu$. When the concentration of $ZnS{{O}_{4}}$ is 1.0 M and that of $CuS{{O}_{4}}$ is 0.01 M, the emf changed to ${{E}_{2}}$. What is the relationship between ${{E}_{{}}}$ and ${{E}_{2}}$
The standard emf for the given cell reaction $Zn+C{{u}^{2+}}=Cu+Z{{n}^{2+}}$ is 1.10 V at ${{25}^{o}}C$. The emf for the cell reaction, when 0.1 M $C{{u}^{2+}}$ and 0.1 M$Z{{n}^{2+}}$ solutions are used, at ${{25}^{o}}C$ is
The emf of a galvanic cell constituting couples of $Z{{n}^{2+}}/Zn\,(0.76\,V)$ and $C{{u}^{2+}}/Cu\,(-0.34\,V)$ is
The standard electrode potential of the half cells are given below $Z{{n}^{2+}}+2{{e}^{-}}\to Zn;\,E=-7.62\,V$, $F{{e}^{2+}}+2{{e}^{-}}\to Fe;\,E=-7.81\,V$ The emf of the cell $F{{e}^{2+}}+Zn\to Z{{n}^{2+}}+Fe$ is
The oxidation potentials of following half-cell reactions are given $Zn\to Z{{n}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=0.76\,V$ $Fe\to F{{e}^{2+}}+2{{e}^{-}};\,{{E}^{0}}=0.44\,V$ what will be the emf of cell, whose cell reaction is $F{{e}^{2+}}(aq)+Zn\to Z{{n}^{2+}}(aq)+Fe$
When copper turnings are added to silver nitrate solution, a blue coloured solution is formed after some time. It is because, copper
Four colourless salt solutions are placed in separate test tubes and a strip of copper is placed in each. Which solution finally turns blue

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