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Calculate the e.m.f. of the cell in whic...

Calculate the e.m.f. of the cell in which the following reaction takes place.
`Ni_((s)) + 2Ag_((0.002M))^(+) to Ni_((0.160M))^(2+) + 2Ag_((s)) , "Given " E_("cell")^@ = 1.05 V `

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Using Nernst equation ,
`E_("cell") = E_("cell")^(@) -(0.0591)/(n) log""([Ni^(+2)])/([Ag^(+)]^(2))`
` = 1.05 - (0.0591)/(2) log ""((0.160))/((0.002)^(2))`
` =1.05 - 0.02955 log 4 xx 104`
=`1.05 - 0.02955( log 10000 + log 4)`
` = 1.05 - 0.02955 ( 4+ 0.6021)`
` E_("cell") = 0.914V`
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SUNSTAR PUBLICATION-II PUC CHEMISTRY ( ANNUAL EXAM QUESTION PAPER MARCH - 2020)-PART-D
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