Problem: When a solution containing M(NO3)2 of an unknown metal M is electrolyzed, it takes 74.1 s for a current of 2.00 A to plate out 0.0737 g of the metal. The metal isa. Cub. Znc. Mnd. Moe. Pd

FREE Expert Solution

For this problem, we are being asked to identify the metal present in M(NO3)2 when it takes 74.1 s at 2.0 A to electrolyze a 0.0737 g of the sample


In this case, we need to find the moles of metal using the Faraday's constant. Then divide the mass of metal to determine the molar mass.


The molar mass will tell us the identity of the metal.


Notice that M(NO3)2 dissociates as:


M(NO3)(aq)  M2+ (aq) + 2 NO3(aq)


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Problem Details

When a solution containing M(NO3)2 of an unknown metal M is electrolyzed, it takes 74.1 s for a current of 2.00 A to plate out 0.0737 g of the metal. The metal is

a. Cu

b. Zn

c. Mn

d. Mo

e. Pd

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