The following reaction occurs spontaneously. 2 H*(aq) + Ca(s) --> Ca²+ (aq) + H₂(g) Write the balanced oxidation half-reaction. A) 2 H*(aq) + 2 e--> H₂(g) B) 2 H(aq)--> H₂(g) + 2 e C) H₂(g) --> 2 H(aq) + 2 e D) Ca(s) + 2 e-> Ca²+ (aq) E) Ca(s)--> Ca2+ (aq) + 2 e B d

The following reaction occurs spontaneously. 2 H(aq) + Ca(s) --> Ca²+ (aq) + H₂(g) Write the balanced oxidation half-reaction. A) 2 H(aq) + 2 e--> H₂(g) B) 2 H(aq)--> H₂(g) + 2 e C) H₂(g) --> 2 H(aq) + 2 e D) Ca(s) + 2 e-> Ca²+ (aq) E) Ca(s)--> Ca2+ (aq) + 2 e B d

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.11QAP

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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.

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20.3a 8

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Question 8
The following reaction occurs spontaneously.
2 H*(aq) + Ca(s) --> Ca²+ (aq) + H₂(g)
Write the balanced oxidation half-reaction.
A) 2 H*(aq) + 2 e
-->
H₂(g)
B) 2 H(aq) --> H₂(g) + 2 e
C) H₂(g) --> 2 H+ (aq) + 2 e
D) Ca(s) + 2 e-> Ca²+ (aq)
a
E) Ca(s)--> Ca2+ (aq) + 2 e

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