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Given the balanced electrochemical reaction below (M and N represent generic metals), what is the [M3+], in moles per liter, required to generate a cell potential (Ecell) of 0.588 V for this reaction at 53.6 °C when [N+] = 1.024 M? Enter your answer to the thousandths place. Do not include units. M(s) + 3N+(aq) → M3+(aq) + 3N(s)       E°cell = 0.572 V

Given the balanced electrochemical reaction below (M and N represent generic metals), what is the [M3+], in moles per liter, required to generate a cell potential (Ecell) of 0.588 V for this reaction at 53.6 °C when [N+] = 1.024 M? Enter your answer to the thousandths place. Do not include units. M(s) + 3N+(aq) → M3+(aq) + 3N(s)       E°cell = 0.572 V

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter19: Applications Of Standard Electrode Potentials
Section: Chapter Questions
Problem 19.8QAP
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Given the balanced electrochemical reaction below (M and N represent generic metals), what is the [M3+], in moles per liter, required to generate a cell potential (Ecell) of 0.588 V for this reaction at 53.6 °C when [N+] = 1.024 M? Enter your answer to the thousandths place. Do not include units.

M(s) + 3N+(aq) → M3+(aq) + 3N(s)       E°cell = 0.572 V

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