![]() Therefore, every mole of Cu plated out requires two moles of electrons.ġ.573663 mol x 2 = 3.147326 mol e¯ requiredģ) Convert moles of electrons to Coulombs of charge:ģ.147326 mol e¯ x 96,485.309 C/mol = 3.0367 x 10 5 CĮxample #2: How many minutes will take to plate out 40.00 g of Ni form a solution of NiSO 4 using a current of 3.450 amp?Ĥ0.00 g divided by 58.6934 g/mole = 0.6815076 mol ![]() General note: I kept all the digits on my calculator I rounded off to the final answer at the end of each problem.Įxample #1: Calculate the quantity of electricity (Coulombs) necessary to deposit 100.00 g of copper from a CuSO 4 solution.ġ00.00 g divided by 63.546 g/mole = 1.573663 molĢ) Determine moles of electrons required: ![]()
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