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m_a_m_a [10]
3 years ago
14

I know that the answer is C. 8, but can you explain step by step how to get that answer?

Chemistry
1 answer:
Leya [2.2K]3 years ago
4 0

Answer:

8

Explanation:

Oxidation:

Fe^{2+} -->Fe^{3+}+e^{-}

Reduction:

Cr_{2}O_{7}^{2-}+6e^{-} -->2Cr^{3+}

We have to equalise the number  of moles of electrons gained and lost in a redox reaction in order to get a balanced reaction.

Hence we have to multiply the oxidation reaction throughout by 6.

and adding the two half-reactions we obtain:

6Fe^{2+}+Cr_{2}O_{7}^{2-} -->6Fe^{3+}+2Cr^{3+}

Still the total charge and number of oxygen is not balanced.

Since the reaction takes place in acidic conditions, we will add required number of H+ to the appropriate side to balance the charge and add half the amount of H2O to balance the hydrogen atoms.

We add 14 H+ on LHS and 7H2O on RHS to obtain:

6Fe^{2+}+Cr_{2}O_{7}^{2-}+14H^{+} -->6Fe^{3+}+2Cr^{3+}+7H_{2}O

Sum of coefficients of product cations = 6+2 = 8

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