Question

3. A steady electric current is passed through molten MgCl, for exactly 1.00 hour, producing 243 grams of Mg metal. If the same current is passed through molten AICI, for 1.00 hour, what is the mass of Al metal produced?

Answer 1

O. A steady electric current i paseed Through molten. molle for Excactly 1.00 hows., producing 943 grams of Ma. Metal. if the same current is passed through. a molten A163 for 1 houy what is the mose of Al melal produced. And Given data : a: Mass of Mg = 24 gm of my deposited mass of Mg = 243 gm mass of AL = ? molar mase of mg= 84.365 gm/mol molas mase of Al= 26.98 gm/mol Apply Faraday second laws of electrolysis. o calculate the no of moles of mg => 11= w мо|-та n= 243 . 24.305 Im= 9.99 Mol mole Ratio =) mg 62 → mgt2 +2465 mgt2 + 2é MG (08) cs) mole Ratio of my = I mole of my 2 moleope Reauired. AllL3 — 41+3 + 36 - A1+3+36 Al mole Ratio of Al= I moleol Al 3 moleole hequired. CSscanned with CamScanner

Faraday Second law no of moles of mg - nool molee of At mole Ratio of mg mole Rational Al het tea MAL= 9.1972 [nal= 6.60] NA 6 Mol. mase H Al 6.666= W 26.98 gm/mol Iw= 179.6972 gm of All CSScanned with CamScanner