FeSO4+K2Cr2O7+H2SO4+Fe2(SO4)3+Cr2(S O4)3+K2SO4+H2O Please balance the equation through Oxidation number method of redox reaction with the process .How is it balanced with full procedure.

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Explanation:

In every redox process, there is an oxidizing agent (that accepts electrons) and a reducing agent* the looses electrons).

For a moment let us ignore the spectator ions and focus on Fe^2+, Cr2O7^2- and H^+.

Hence,

Reduction half equation;

Cr2O7^2-(aq) + 14H^+(aq) + 6e > 2Cr^+(aq) + 7H2O(l)

Oxidation half equation;

6Fe^2+(aq) > 6Fe^3+(aq) + 6e

Overall redox reaction equation;

Cr2O7^2-(aq) + 14H^+(aq) + 6Fe^2+(aq) >2Cr^+(aq) + 6Fe^3+(aq)

From here the balanced molecular reaction equation is;

K2Cr2O7(aq) + 6FeSO4(aq) + 7H2SO4(aq) > Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) +  7H2O(l)

step-by-step explanation:

whole numbers, zero or greater

it is reliable if two scientists recorded it