Consider the electrochemical reaction between Ag(s) and Cl_{2(g)} electrodes in 1 litre of 0.1 M KCl aqueous solution. Solubility product of AgCl is 1.8\times10^{-10} and F = 96500 C/mol. At 1 µA current, calculate the time required to start observing the AgCl precipitation in the galvanic cell

KEAM 2018 Physics and Chemistry Paper

Question : 113 of 120

Marks: +1, -0

Consider the electrochemical reaction between Ag(s) and Cl2(g) electrodes in 1 litre of 0.1 M KCl aqueous solution. Solubility product of AgCl is 1.8×10−10 and F = 96500 C/mol. At 1 µA current, calculate the time required to start observing the AgCl precipitation in the galvanic cell

173 s
346 s
1.25×106 s
1.25×105 s
101 s

Validate

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