Practice Problem Submissions are not permanently recorded Balance thefollowing r

Question

Practice Problem Submissions are not permanently recorded Balance thefollowing redox reaction and enter the correct coefficients for all of the species in the balanced reaction H2S + Fe3 + Fe2+ + S (s) This reaction takes place in an acidic solution 1H2S 12 Fe3+ 2 Fe2+ 1 S (s) Divide the reaction into two half-reactions, then balance each half-reaction Balance oxygen first, by adding water Balance hydrogen next, using protons. Finally, balance charge, using electrons. The number of electrons consumed (reduction half-reaction) must equal the number of electrons produced (oxidation half-reaction) Since this reaction takes place in an acidic solution there may be excess acid on one or the other sides of the equation Submit AsverIncorrect.

Explanation / Answer

   H2S + Fe+3 --------------- Fe+2 + S

      -2      +3                       +2       0

oxidatio half reaction                         reduction half reaction                

H2S ---------------- S                                         Fe+3 ------------------ Fe+2

H2S -------------- S + 2 H+                               Fe+3 + e- ----------- Fe+2

H2S -------------- S   + 2 H+ + 2e-

[ H2S ----------- S + 2 H+ + 2e-] x1

[ Fe+3 + e- -------- Fe+2] x2

H2S ------------- S + 2 H+ + 2e-

2Fe+3 + 2e- ------------ 2 Fe+2

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H2S + 2 Fe+3 ----------------- 2 Fe+2 + S + 2 H+

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The net equation is H2S + 2 Fe+3 ----------------- 2 Fe+2 + S + 2 H+.

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