(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
Question
I need solutions please, avoid using Ai
![(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%2Fe87f1b40-d40c-44ae-8262-47c66e4e833e%2F4fd634a1-3e66-47f3-bdf7-7378d8516123%2F0q88lha_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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