Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......
(N/A) $1$. The strongest reducing agent in aqueous solution is $Li$ (Lithium) due to its high hydration energy and low sublimation energy.
$2$. The strongest oxidizing agent among gases is $F_2$ (Fluorine) gas.
$3$. The standard reduction potential of any electrode is measured with reference to the Standard Hydrogen Electrode $(SHE)$,which is assigned a potential of $0.00 \ V$.
$2$. The strongest oxidizing agent among gases is $F_2$ (Fluorine) gas.
$3$. The standard reduction potential of any electrode is measured with reference to the Standard Hydrogen Electrode $(SHE)$,which is assigned a potential of $0.00 \ V$.
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View SolutionGiven $:$
$(i) \, Cu^{2+} + 2e^- \rightarrow Cu \,, \, E^o = 0.337 \, V$
$(ii) \, Cu^{2+} + e^- \rightarrow Cu^{+} \,, \, E^o = 0.153 \, V$
Electrode potential,$E^o$ for the reaction,
$Cu^{+} + e^- \rightarrow Cu \,,$ will be $............$ $V$.
$(i) \, Cu^{2+} + 2e^- \rightarrow Cu \,, \, E^o = 0.337 \, V$
$(ii) \, Cu^{2+} + e^- \rightarrow Cu^{+} \,, \, E^o = 0.153 \, V$
Electrode potential,$E^o$ for the reaction,
$Cu^{+} + e^- \rightarrow Cu \,,$ will be $............$ $V$.
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