In a redox change $$Ba(MnO4)2$$ oxidizes $$K4$$[$$Fe(CN)6$$] into $$K+$$, $$Fe3+$$, $$CO32$$− and $$NO3$$− ions in acidic medium, it self being reduced to $$Mn2+ions$$. How many moles of $$Ba(MnO4)2are$$ reduced by $$1$$ mole of $$K4Fe(CN)6$$ ?

Question

In a redox change  $$Ba(MnO4)2$$ oxidizes $$K4$$[$$Fe(CN)6$$] into $$K+$$,  $$Fe3+$$,  $$CO32$$− and $$NO3$$− ions in acidic medium, it self being reduced to $$Mn2+ions$$. How many moles of  $$Ba(MnO4)2are$$ reduced by $$1$$ mole of $$K4Fe(CN)6$$ ?

Infinity Learn · Accepted Answer

$$10e+$$ $$Mg3++$$→ $$2Mn2+$$]×$$61$$                                (Fe2+)→ $$Fe3++e$$                               $$(C2+)6$$ → $$6C4++12e$$                                $$(N3-)6$$ → $$6N5++48eFe2++C2++N3$$−→ $$Fe3++C4++N5++61e$$] ×  $$10$$¯$$61$$ $$Ba(MnO4)2+10K4$$[$$Fe(CN)6$$]→ $$122Mn2++Fe3++6C4++6N5+$$∵$$10$$ mole $$K4Fe(CN)6$$≡$$61$$ mole $$BaMnO42$$∴$$1$$ mole $$K4Fe(CN)6$$≡$$6.1$$ mole $$Ba(MnO$$ $$42$$

In a redox change Ba(MnO4)2 oxidizes K4[Fe(CN)6] into K+, Fe3+, CO32− and NO3− ions in acidic medium, it self being reduced to Mn2+ions. How many moles of Ba(MnO4)2are reduced by 1 mole of K4Fe(CN)6 ?

Detailed Solution

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