The first reaction you will be performing is the reduction of the permanganate ion MnO4– by the iron (II) ion Fe2+ in acidic conditions to standardize the concentration of the perman- ganate solution; the unbalanced chemical equation for the reaction is MnO4– (aq) + Fe2+ (aq) → Mn2+ (aq) + Fe3+ (aq) (a) Split the unbalanced equation into two half-reactions, one for the permanganate ion and one for the iron (II) ion, and write them out. (b) For every one permanganate ion reacted, how many electrons are transferred? (c) For every one iron (II) ion reacted, how many electrons are transferred? (d) In the balanced balanced chemical equation for the redox reaction, how many electrons are transferred per mole of permanganate ions? (e) How many moles of iron (II) ions are necessary to completely react one mole of perman- ganate ions?
The first reaction you will be performing is the reduction of the permanganate ion MnO4– by the iron (II) ion Fe2+ in acidic conditions to standardize the concentration of the perman- ganate solution; the unbalanced chemical equation for the reaction is
MnO4– (aq) + Fe2+ (aq) → Mn2+ (aq) + Fe3+ (aq)
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(a) Split the unbalanced equation into two half-reactions, one for the permanganate ion and
one for the iron (II) ion, and write them out.
-
(b) For every one permanganate ion reacted, how many electrons are transferred?
-
(c) For every one iron (II) ion reacted, how many electrons are transferred?
-
(d) In the balanced balanced chemical equation for the
redox reaction , how many electrons are transferred per mole of permanganate ions? -
(e) How many moles of iron (II) ions are necessary to completely react one mole of perman- ganate ions?
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