Chapter 20, Problem 91a
(a) A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days?
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(c) What process occurs at the anode in the electrolysis of molten NaCl?
(d) Why is sodium metal not obtained when an aqueous solution of NaCl undergoes electrolysis?
(d) Why are active metals such as Al obtained by electrolysis using molten salts rather than aqueous solutions?
(a) Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 * 104 A flowing for a period of 24 h. Assume the electrolytic cell is 85% efficient. (b) What is the minimum voltage required to drive the reaction?
A disproportionation reaction is an oxidation–reduction reaction in which the same substance is oxidized and reduced. Complete and balance the following disproportionation reactions: (b) MnO42-(aq) → MnO4-(aq) + MnO2(s) (acidic solution)