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Q.

How many grams of Cr are deposited in the electrolysis of solution of $Cr {({NO}_{3})}_{3}$ in the same time that it takes to deposit 0.54 g of Ag in a silver coulometer arranged in series with the $Cr {({NO}_{3})}_{3}$ cell?(Atomic mass: Cr = 52.0; Ag=108)

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a

0.0866

b

0.220

c

0.0288

d

0.173

answer is A.

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Detailed Solution

$No . of equivalents of Ag = \frac{0.54}{108} = No . of equivalents of Cr = \frac{W_{Cr}}{52} \times 3 ∴ W_{Cr} = \frac{0.54}{108} \times \frac{52}{3} = 0.0866$

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How many grams of Cr are deposited in the electrolysis of solution of CrNO33 in the same time that it takes to deposit 0.54 g of Ag in a silver coulometer arranged in series with the CrNO33cell?(Atomic mass: Cr = 52.0; Ag=108)