Calculate the cell potential for the following reaction as written at 25.00 Â°C, given that [Zn2...

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Chemistry

Calculate the cell potential for the following reaction aswritten at 25.00 Â°C, given that [Zn2 ] = 0.763 M and [Sn2 ] =0.0140 M. Standard reduction potentials can be found here.
Zn(s)+SN²⁺ YIELDS Zn²⁺(aq)+Sn(s)

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4.1 Ratings (683 Votes)

As in the given problem

Zn(s)+Sn²⁺ -------------> Zn²⁺(aq)+Sn(s)

Zinc oxidized and tin reduces

Zinc will act as an anode and tin as a cathode

Than standard reduction potential of the cell = E^o cathode- E^o Anode

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = -0.14 â€“ (-0.76) (from electrochemical series)

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 0.62 volts

E _cell = E^o_cell â€“ RT/nF log [con of oxidized form] /[con of reduced form]

Â Â Â Â Â Â Â Â = 0.62 â€“ 0.0591/2 log (0.763/ 0.0140)

Â Â Â Â Â Â Â Â = 0.62 â€“ 0.0591/2 log 54.4

Â Â Â Â Â Â Â Â = 0.62 - 0.02955 X 1.73

Â Â Â Â Â Â Â Â = 0.62 - 0.0512

Â Â Â Â = 0.5688 volts

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