Consider the battery.Cd(s) | CdCl, (aq) || CI¯(aq) | Cl, (1) | C(s)Write the reduction half-reaction occuring at the C(s) electrode. Include physical states.C(s) electrode: Cl, (1) + 2e-→ 2C1-(aq)E°= 1.4 VFrom which electrode will electrons flow from the battery into a circuit?C(s) electrodeCd(s) electrodeCalculate the mass of Cl, consumed if the battery delivers a constant current of 573 A for 60.0 min.126kgmass:Incorrect

All the above answer is correct so, solving only last part, the mass of Cl2

Answered: Calculate the mass of Cl₂ consumed if…

Calculate the mass of Cl₂ consumed if the battery delivers a constant current of 573 A for 60.0 min. mass: 126 Incorrect kg

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

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Concept explainers

Electrolysis

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 electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Consider the battery.
Cd(s) | CdCl, (aq) || CI¯(aq) | Cl, (1) | C(s)
Write the reduction half-reaction occuring at the C(s) electrode. Include physical states.
C(s) electrode: Cl, (1) + 2e-
→ 2C1-(aq)
E°
= 1.4 V
From which electrode will electrons flow from the battery into a circuit?
C(s) electrode
Cd(s) electrode
Calculate the mass of Cl, consumed if the battery delivers a constant current of 573 A for 60.0 min.
126
kg
mass:
Incorrect

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