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(D) The balanced chemical equation for the reaction in acidic medium is: $Cr_2O_7^{2-} + 14H^+ + 6Fe^{2+} 	o 2Cr^{3+} + 6Fe^{3+} + 7H_2O$From the sto

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$6$

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(D) The balanced chemical equation for the reaction in acidic medium is: $Cr_2O_7^{2-} + 14H^+ + 6Fe^{2+} 	o 2Cr^{3+} + 6Fe^{3+} + 7H_2O$From the stoichiometry of the reaction,$1 	ext{ mole}$ of $K_2Cr_2O_7$ reacts with $6 	ext{ moles}$ of $FeSO_4$.Alternatively,using the concept of equivalents:$	ext{Equivalents of } K_2Cr_2O_7 = 	ext{Equivalents of } FeSO_4$$n 	ext{-factor of } K_2Cr_2O_7 	imes 	ext{moles} = n 	ext{-factor of } FeSO_4 	imes 	ext{moles}$$6 	imes 1 = 1 	imes x$$x = 6 	ext{ moles}$.

One mole of potassium dichromate completely oxidises the following number of moles of ferrous sulphate in acidic medium.

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