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21 February, 20:21

The chemical reaction represented by the following balanced chemical equation takes place in aqueous

solution: MnO4 + 5 Fe2+8H - Mn2 + 5 Fe3 + 4H2O

When the disappearance of the permanganate ion, MnO4, is monitored, the rate of reaction for the

consumption of the ion is 4.0x10^2 mol/L. s. Calculate the reaction rate for all other reactants and products.

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  1. 21 February, 22:19
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    Fe²⁺ = 80mol/Ls

    H⁺ = 50mol/Ls

    Mn²⁺ = 4.0x10²mol/Ls

    Fe³⁺ = 80mol/Ls

    H₂O = 1.0x10²mol/Ls

    Explanation:

    Based on the reaction:

    MnO₄⁻ + 5 Fe²⁺ + 8H⁺ → Mn²⁺ + 5 Fe³⁺ + 4H₂O

    Where 1 mole of permangante with 5 moles of Fe²⁺ and 8 moles of H⁺ produce 1 mole Mn²⁺, 5 of Fe³⁺ and 4 of H₂O

    If the diappearence of 1 mole has a rate of 4.0x10²mol/Ls, disappearence of 5 moles of Fe²⁺ and 8 moles of H⁺ have a rate of:

    Fe²⁺ = 1 mole MnO₄⁻ * (4.0x10²mol/Ls / 5 moles of Fe²⁺) = 80mol/Ls

    H⁺ = 1 mole MnO₄⁻ * (4.0x10²mol/Ls / 8 moles of H⁺) = 50mol/Ls

    And rate of appearance of 1 mole Mn²⁺, 5 of Fe³⁺ and 4 of H₂O are:

    Mn²⁺ = 1 mole MnO₄⁻ * (4.0x10²mol/Ls / 1 moles of Mn²⁺) = 4.0x10²mol/Ls

    Fe³⁺ = 1 mole MnO₄⁻ * (4.0x10²mol/Ls / 5 moles of Fe³⁺) = 80mol/Ls

    H₂O = 1 mole MnO₄⁻ * (4.0x10²mol/Ls / 4 moles of H₂O) = 1.0x10²mol/Ls
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