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Chemistry Tough Question Unit 5 Edexcel

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    • Thread Starter

    So it starts of pretty straightforward....

    (b) Vanadium ions exist in oxidation states from (V) to (II). (i) Use your data booklet (page 15) to find the standard electrode (reduction) potential for the reduction of vanadium(IV), VO2+, to vanadium(III), V3+.

    So I looked the value up and it is +0.34V

    The next part though....

    This is June 2010 Q23 btw
    Use your answer to (b)(i), and the data below, to calculate E○ cell for the formation of vanadium(V) and vanadium(III) from vanadium(IV) in acidic solution. State if the reaction is feasible under standard conditions and justify your answer. VO2+(aq) + 2H+(aq) + e– VO2+(aq) + H2O(l) E○ = + 1.00 V


    I worked the answer out as 0.66V but the answer says -0.66V

    WHy is there a negative!!!!

    (Is it something to do with the fact it is a disproportionation reaction )

    Chemistry is so frustrating
    • Thread Starter

    I get it!!!!! dw people
Updated: May 8, 2016
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