An electrochemical cell is based on the following two half-reactions: oxidation: Sn (s) →Sn²+ (aq, 1.90 M)+2e¯ reduction: ClO₂ (g, 0.200 atm )+e¯→ClO₂ (aq, 2.00 M)
An electrochemical cell is based on the following two half-reactions: oxidation: Sn (s) →Sn²+ (aq, 1.90 M)+2e¯ reduction: ClO₂ (g, 0.200 atm )+e¯→ClO₂ (aq, 2.00 M)
Chapter19: Applications Of Standard Electrode Potentials
Section: Chapter Questions
Problem 19.8QAP
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Can someone please explain to me why we get 2 ClO2 and 2 ClO2^- instead of 1 each after we balance the reaction?
I already have the equation balanced I just want to know why it ends up that way.
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