Course Contents Set 28: Electrochemistry half reactions + O TimerNotes Evaluate

Question

Course Contents Set 28: Electrochemistry half reactions + O TimerNotes Evaluate Feedback PrintI Iron(II) ion, reacts with permanganate lon, in acidic solution to produce ironkil) on and manganesel lI) ion If exactly 30.0 mL of an Fe2 solution? solution is required to react completely with 35.0 ml of a 0.0550 M permanganate solution, what is the molarity bi the Fe? (Number only) Submit Answer Tries 1/12 Previous Tries Threaded Vies Chronological View Other ViewS Export NEW Ellen Mitchell Reply (Thu Apr 5 04:38:59 pm 2018 (EDT)) You will first need to balance this REDOx reaction before you can solve the stolchiometry problem. You do not need a completely balanced reaction when you begin. Just write out the reactant specles given > product species given. The H and O will balance once you add your H20 and H+ in the balancing process Your text book p. 177 (4th ed. Tro) shows the hierarchy of assigning oxidation states, most of these are intuitive based on our knowledge of all I ions form + 1 lons and so on even make the list so when looking to assign oxidation numbers of a compound with C and O, Assign 02- and then whatever C must be. However, it is useful to note that the precedence of oxidation states of 02-C where C? does not

Explanation / Answer

Fe+2(aq) + MnO4-(aq) -------------- Fe+3(aq) + Mn+2(aq)

The balanced equation is

5 Fe+2(aq) + MnO4-(aq) + 8 H+(aq) -------------- 5 Fe+3(aq) + Mn+2(aq) + 4 H2O(l)

5 mole            1 mole

         Fe+2                                             MnO4-

M1=                                          M2 = 0.0550M

V1= 30.0ml                                V2= 35.0ml

n1= 5 mole                                 n2= 1 mole    ( number of moles are getting from the balanced equation)

      M1V1/n1= M2V2/n2

M1x30.0/5 = 0.0550x35.0/1

M1 = 0.3208M

Molarity of Fe+2 ion = 0.321M

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