Question

19 points:

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.

Answer 1

Answer:

Explanation:

MnO₄⁻ + 5 Fe2⁺ + 8H⁺ = Mn⁺² + 5Fe⁺³ + 4H₂O.

- d [MnO₄⁻ ] / dt = 4 x 10² mol /L.s.

- [ Fe²⁺ ] / dt = 5 x - d [MnO₄⁻ ] / dt

= 5 x 4 x 10² mol /L.s.

20 x 10²

- d [ H⁺] / dt = 8 x - d [MnO₄⁻ ] / dt

= 8 x  4 x 10²

= 32 x 10² mol /L.s.

+d [ Mn⁺² ] / dt = - d [MnO₄⁻ ] / dt

= 4 x 10² mol /L.s

+d [ Fe⁺³ ] / dt = 5 x - d [MnO₄⁻ ] / dt

= 20 x 10² mol /L.s