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Question
Calculate the value of Ecell at 298 K for the following cell:
`(Al)/(Al^(3+)) (0.01M) || Sn^(2+) ((0.015 M))/(Sn)`
`E° _(Al^(3+))/(AI)= -1.66 " Volt and " E° _(Sn^(2+)) /(Sn) = -0.14` volt
Solution
`(Al)/(Al^(3+)) (0.01M) || Sn^(2+) ((0.015 M))/(Sn)`
Given, `E° _((AI^(3+))/(AI)) = -1.66V,`
`E° _((Sn^(2+))/(Sn)) = -0.14V,`
`E°_(cell) = E°_R - E°_L`
=-0.14 - (-1.66)
=-0.14 + 1.66=1.52 V
Cell reaction is:
2AI + 3Sn2+ → 2AI3+ + 3Sn and n = 6
According to Nernst equation, at 298 K
`E_(cell) = E°_(cell) - 0.059/n log ([AI^(3+)]^2)/([Sn^(2+)]^3)`
`=1.52 - 0.059/6 log ([0.01]^2)/([0.015]^3) = 1.52 -0.01447`
`E_(cell) = 1.50553` V.
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