A) \[\left[ \text{F}{{\text{L}}^{\text{2}}}{{T}^{-\text{2}}} \right]\]
B) \[\left[ \text{F}{{\text{L}}^{-\text{1}}}{{\text{T}}^{\text{2}}} \right]\]
C) \[\left[ {{\text{F}}^{2}}\text{L}{{\text{T}}^{\text{-2}}} \right]\]
D) \[-\text{273}.\text{15}{}^\circ \text{F}\]
Correct Answer: A
Solution :
\[Zn\xrightarrow{{}}Z{{n}^{2+}}+2{{e}^{-}}\] (oxidation half- reaction) \[C{{u}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Cu\] (reduction half- reaction) Emf of the cell = standard oxidation potential of zinc electrode + standard reduction potential of Cu electrode \[[{{m}^{0}}{{L}^{-1}}{{T}^{-2}}]\]
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