c D www.webassign netwebstudent/Assignment Responses/sul 15076130 bmit?dep Hstra

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c D www.webassign netwebstudent/Assignment Responses/sul 15076130 bmit?dep Hstrategy video In an electrolytic cell, the electrolysis of an aqueous zinc solution results in the deposition of zinc at the cathode. If a current of 1184 A is used, how much time will be needed to plate out 0.329 mol Zn(s)? Did you recall the equation that relates the amount of charge passing through an electrolytic cell to the quantity of electric current passing through the cell within a certain time period? Did you recall the meaning of y's constant? Did you recall how to use the stoichiometry of a balanced equation to calculate the meles reactant? of a upporting Materials periodic Table Constants and supplemental Data standard Electrode Additional Material Section 17.7 Tutorial Submit Answer Save Progress Practice Another Vorsion My Notes o Ask your wache 177 WA 008, osios points I Previous Asswera osGenChem a a O Ask me anything

Explanation / Answer

mass of Zn = no of moles * gram molar mass

                    = 0.329*65.4   = 21.52g

c                   = 118.4A

M                 = 65.4g/mole

Zn+2 + 2e- -----> Zn

        Z= 2

      F = 96500C

W   = MCt/ZF

t = WZF/MC

       = 21.52*2*96500/65.4*118.4   = 536.376sec >>> answer

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