Qstnid -I-5- Calculate The Emf Of The Cell In Which The Following Reaction Takes Place: <Img Src="\etl\image\esa-cbse-xii\chem-hwh-sb1\c03/1_m40455851.gif" Width="329" Height="28"> Given That <Img Src="\etl\image\esa-cbse-xii\chem-hwh-sb1\c03/1_e96fdf6.gif" Width="36" Height="28">= 1.05 V - 03: Electrochemistry - Neet-xii-chemistry

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NEET-XII-Chemistry

03: Electrochemistry

Qstn# I-5 Prvs-Qstn Next-Qstn

#5
Calculate the emf of the cell in which the following reaction takes place:

Given that = 1.05 V

Ans : Applying Nernst equation we have:

= 1.05 - 0.02955 log 4 × 10⁴

= 1.05 - 0.02955 (log 10000 + log 4)

= 1.05 - 0.02955 (4 + 0.6021)

= 0.914 V