Balance Equation and Net Ionic Equation. What are the reducing agent and oxidizi

Question

Balance Equation and Net Ionic Equation. What are the reducing agent and oxidizing agent. 7a)MNO4-+Fe+2 --->Fe+3+ Mn+2 7b)MnO4-+Cr2O-4---->Mn+2+CO2 Balance Equation and Net Ionic Equation. What are the reducing agent and oxidizing agent. 7a)MNO4-+Fe+2 --->Fe+3+ Mn+2 7b)MnO4-+Cr2O-4---->Mn+2+CO2 7b)MnO4-+Cr2O-4---->Mn+2+CO2

Explanation / Answer

a) Fe2+ => Fe3+ +e-                  MnO4- + 5e- => Mn2+         (MnO4- has Mnin 7+ oxidation state, so need 5 electrons) MnO4- + 5e- => Mn2+ + 4H2O   (add 4 H2O for 4O's; balancing MnO4 MnO4- + 5e- + 8H+ => Mn2+ +4H2O       Add both equations, eliminating electrons 5Fe2+ + MnO4- + 8H+ => 5Fe3+   + Mn2+ + 4H2O oxidizing agent: MnO4- (it gets reduced) reducing agent Fe2+ (it gets oxidized) b) Can't finish the second one. I think you put the wrong equation.You shouldn't be forming CO2, but a chromium product. Please fixthis and then PM me (I won't be notified of the fix unless youPM)

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