Chemistry

Balance the following equation for a half reaction that occurs in acidic solution. Use e– as the symbol for an electron.

U^4+ --> UO2^+

There is a hint: In acidic solution, you may add H2O and H as needed to balance oxygen and hydrogen. When finished, don\'t forget to balance the charge by adding e– as needed.

But it makes no sense to me. Could someone please help me?

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  1. I wonder if that is [UO2]^2+?
    U^4+ ==> UO2^+
    Here is how I do it which is not the short way.
    Oxidation state of U on left is +4. On right is +5. Balance the change in oxidation state by adding electrons to the appropriate side.
    U^4+ ==> UO2^+ + e

    Count the charge on the left and right. +4 on the left; zero on the right so we add H^+ to the right to balanced the charge.
    U^4+ ==> UO2^+ + e + 4H^+
    Then add H2O to the other side to balance.
    U^4+ + 2H2O ==> UO2^+ + e + 4H^+

    but I really think you meant for that ion on the right to be [UO2]^2+

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