Consider an electrolytic cell with a steady current of 169 amperes which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 31) + 3C (s) -4AI +3CO (s) 2(g) What is the time, in hours, needed to produce 218 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.

Consider an electrolytic cell with a steady current of 169 amperes which produces Al(s) (atomic mass = 26.98 g/mol) according to the equation below. 2A1,0 31) + 3C (s) -4AI +3CO (s) 2(g) What is the time, in hours, needed to produce 218 g of Al(s)? Show your answers in two decimal places. Do NOT include units in your final answer.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 84QRT

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