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Suppose a current of 220.mA is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 79.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

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Answer:

0.0195 g

Explanation:

Ag^+(aq) + e -------> Ag(s)

Since 1 electron was transferred, that means 96500C of electricity was required

108 g is deposited 96500 C

xg is deposited 220 × 10^-3 × 79.0

x = 108 × 220 × 10^-3 × 79.0/96500

x= 19.5 × 10^-3 g

x= 0.0195 g

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