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प्रश्न
Answer the following:
Predict whether the following reaction would occur spontaneously under standard state condition.
`2"Br"_(("aq"))^(-) + "Sn"_(("aq"))^(2+) -> "Br"_(2("l")) + "Sn"_(("s"))`
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उत्तर
`2"Br"_(("aq"))^(-) + "Sn"_(("aq"))^(2+) -> "Br"_(2("l")) + "Sn"_(("s"))`
At anode: `2"Br"_(("aq"))^(-) -> "Br"_(2("l")) + 2"e"^(-)`
At cathode: `"Sn"_(("aq"))^(2+) + 2"e"^(-) -> "Sn"_(("s"))`
From the electrochemical series we have,
`"E"_("Br"_2)^circ` = 1.080 V and `"E"_"Sn"^circ` = - 0.136 V
For cell having `"Br"_(2("l"))` as anode and Sn as cathode.
`"E"_"cell"^circ = "E"_"Sn"^circ - "E"_("Br"_2)^circ`
= - 0.136 V - 1.080 V
`"E"_"cell"^circ` = - 1.216 V
Emf of cell being negative, the given cell reaction is nonspontaneous.
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संबंधित प्रश्न
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| Element | `"E"^0 ("V")` |
| Al | −1.66 |
| Fe | −0.44 |
| Hg | +0.79 |
| Cu | +0.337 |
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if \[\ce{E^0_{Ni}}\] = −0.25 V, \[\ce{E^0_{Au}}\] = 1.50 V.
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if \[\ce{E{^{\circ}_{Ni}}}\] = −0.25 V and \[\ce{E{^{\circ}_{Al}}}\] = −1.66 V?
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If \[\mathrm{E^o\left(Cd_{(aq)}^{+2}|Cd_{(s)}\right)=-0.40~V}\]. What is potential for \[\mathrm{Cd}_{(s)}\xrightarrow{}\mathrm{Cd}_{(aq)}^{+2}\left(0.01\mathrm{M}\right)+2\mathrm{e}^{-}\] at 298 K?
Which from following formulae is used to obtain value of E°cell for a reaction taking place in Dry cell?
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