(c) The E.M.F of a cell corresponding to the reaction at 1.0atm is 0.30V and 250C. From the equation below: Zn(s) + 2H+ aq Zna(0.1m) H2(g) i. ii. Write the half cell reaction for both oxidation and reduction Calculate the pH of the hydrogen electrode [Ecell = -0.76V]
(c) The E.M.F of a cell corresponding to the reaction at 1.0atm is 0.30V and 250C. From the equation below: Zn(s) + 2H+ aq Zna(0.1m) H2(g) i. ii. Write the half cell reaction for both oxidation and reduction Calculate the pH of the hydrogen electrode [Ecell = -0.76V]
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![(c) The E.M.F of a cell corresponding to the reaction at 1.0atm is 0.30V and 250C. From the
equation below: Zn(s) + 2H+ aq
Zna(0.1m) H2(g)
i.
ii.
Write the half cell reaction for both oxidation and reduction
Calculate the pH of the hydrogen electrode [Ecell = -0.76V]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb56f47c5-8801-486e-9908-a34ae3fd08c0%2F1b46e13e-b0f7-484e-b057-970e318442a7%2Fiidmexn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(c) The E.M.F of a cell corresponding to the reaction at 1.0atm is 0.30V and 250C. From the
equation below: Zn(s) + 2H+ aq
Zna(0.1m) H2(g)
i.
ii.
Write the half cell reaction for both oxidation and reduction
Calculate the pH of the hydrogen electrode [Ecell = -0.76V]
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