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प्रश्न
Answer the following in one or two sentences.
What is the standard cell potential for the reaction?
\[\ce{2Al(s) + 3Ni^{2⊕}(1M) -> 2Al^{3⊕}(1 M) + 3Ni(s)}\]
if `"E"_"Ni"^0` = −0.25 V and `"E"_"Al"^0` = −1.66 V
उत्तर
Given: `"E"_"Ni"^0` = −0.25 V, `"E"_"Al"^0` = −1.66 V
To find: Standard cell potential
Formula: `"E"_"cell"^0 = "E"_"cathode"^0 - "E"_"anode"^0`
Calculation: Electrode reactions are
At anode: \[\ce{Al_{(s)} -> Al^{3+}_{( aq)} + 3e^-}\]
At cathode: \[\ce{Ni^{2+}_{ (aq)} + 2e^- -> Ni_{(s)}}\]
The standard electrode potential is given by
`"E"_"cell"^0 = "E"_"cathode"^0 - "E"_"anode"^0`
`"E"_"cell"^0 = "E"_"Ni"^0 - "E"_"Al"^0`
= (–0.25 V) – (−1.66 V)
= 1.41 V
The standard cell potential for the reaction is 1.41 V.
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संबंधित प्रश्न
Answer the following in one or two sentences.
What is standard cell potential for the reaction
\[\ce{3Ni_{(s)} + 2Al^{3+} (1M) → 3Ni^{2+} (1M) + 2Al(s)}\], if `E_"Ni"^circ` = –0.25 V and `"E"_("Al")^circ` = –1.66 V?
Answer the following in brief.
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Answer the following:
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E°Zn = −076V, E°Cr = −0.74V.
Answer the following:
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| Element | `"E"^0 ("V")` |
| Al | −1.66 |
| Fe | −0.44 |
| Hg | +0.79 |
| Cu | +0.337 |
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