Consider the following cell reaction: Zn(s) + 2 H+(? M) —>Zn²+ (1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.416 volts, what is the pH of the hydrogen electrode? pH =
Consider the following cell reaction: Zn(s) + 2 H+(? M) —>Zn²+ (1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.416 volts, what is the pH of the hydrogen electrode? pH =
General Chemistry - Standalone book (MindTap Course List)
11th Edition
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.127QP
Related questions
Question
![Consider the following cell
reaction:
Zn(s) + 2 H+(? M) —>Zn²+
(1.00 M) + H2(g)(1.00 atm)
If the cell potential at 298 K
is 0.416 volts, what is the
pH of the hydrogen
electrode?
pH
=](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcd818504-a262-48c2-8691-4c4f03fb909f%2F9d5ba3a0-a5ee-452f-a92c-3f60492c4b02%2Ffw17i2e_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following cell
reaction:
Zn(s) + 2 H+(? M) —>Zn²+
(1.00 M) + H2(g)(1.00 atm)
If the cell potential at 298 K
is 0.416 volts, what is the
pH of the hydrogen
electrode?
pH
=
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