Answer:
See explanation
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)
