Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an electrochemical process of which one half reaction is Mn2*(aq) + 2H,0(1) → MnO2(s) + 4H*(aq) + 2e If a current of 25.0 A is used, how many hours are needed to produce 1.23 kg of MnO2?

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half-
reaction is
Mn2*(aq) + 2H2O(1)
→ MnO2(s) + 4H*(aq) + 2e
If a current of 25.0 A is used, how many hours are needed to produce 1.23 kg of Mn0,?
hours
8 of 16
...
Nex
Transcribed Image Text:History Bookmarks People Tab Window Help 2021-04- M Inbox (370 X O Dashboarc X 9 Class Sch x banner.ro O Banner ation.com/ext/map/index.html?_con%3Dcon&external_browser%3=0&launchUrl=https%253A%252F%252Fn Saved n Set 3 attempts left Check my work Enter your answer in the provided box. The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half- reaction is Mn2*(aq) + 2H2O(1) → MnO2(s) + 4H*(aq) + 2e If a current of 25.0 A is used, how many hours are needed to produce 1.23 kg of Mn0,? hours 8 of 16 ... Nex
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