14th Edition

ISBN: 9781264243709

Author: Chang, Raymond

Publisher: MCGRAW-HILL HIGHER EDUCATION

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Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electroly…

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Chapter 18, Problem 18.119QP

An electrolysis cell was constructed similar to the one shown in Figure 18.18, except 0.1 M MgCl₂(aq) was used as the electrolyte solution. Under these conditions, a clear gas was formed at one electrode and a very pale green gas was formed at the other electrode in roughly equal volumes. (a) What gases are formed at these electrodes? (b) Write balanced half-reactions for each electrode. Account for any deviation from the normally expected results.

Figure 18.18 Apparatus for small-scale electrolysis of water. The volume of hydrogen gas generated at the cathode is twice that of oxygen gas generated at the anode.

Chapter 18, Problem 18.119QP, An electrolysis cell was constructed similar to the one shown in Figure 18.18, except 0.1 M

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Chapter 18, Problem 18.118QP

Chapter 18, Problem 18.120QP

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Chapter 18 Solutions

Chemistry

Ch. 18.1 - Balance the following equation for the reaction in...Ch. 18.1 - Determine the number of electrons transferred in...Ch. 18.1 - For the following reaction in acidic solution,...Ch. 18.2 - Write the cell diagram for the following redox...Ch. 18.2 - Write the balanced redox reaction corresponding to...Ch. 18.3 - Can Sn reduce Zn2+(aq) under standard-state...Ch. 18.3 - What is the standard emf of a galvanic cell made...Ch. 18.3 - Prob. 1RCF Ch. 18.3 - Prob. 2RCF Ch. 18.4 - Prob. 4PE

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Solution Summary: The author explains that the gas formed at each electrode has to be predicted. Electrolysis occurs when electrical energy is used to cause a non-spontaneous chemical reaction.

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Chapter 18 Solutions