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What mass of Cu(s) is electroplated by running 30.0 A of current through a Cu2+(aq) solution...

What mass of Cu(s) is electroplated by running 30.0 A of current through a Cu2+(aq) solution for 4.00 h?

Express your answer to three significant figures and include the appropriate units.

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Part B

How many minutes will it take to electroplate 46.1 g of gold by running 5.00 A of current through a solution of Au+(aq)?

Express your answer to three significant figures and include the appropriate units.

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Expert Solution

W = MCt/ZF

Cu^2+ (aq) + 2e^- -------------> Cu(s)

Z = 2

F = 96500c

C = 30A

t = 4h = 4*60*60 = 14400sec

atomic masss of Cu (M) = 63.5g/mole

W = Mct/ZF

= 63.5*30*14400/2*96500 = 142g

part-B

W = 46.1g

C = 5A

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

Z = 1

F = 96500c

M = 196.96g/mole

W = Mct/ZF

t = WZF/Mc

= 46.1*1*96500/196.96*5 = 4517.3sec

= 4517.3/60 = 75.3minutes >>>>>answer

queen_honey_blossom answered 1 year ago

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