(D) When dichromate ion oxidises $Fe^{2+}$ ions in aqueous acidic medium to $Fe^{3+}$,the following balanced redox reaction takes place:$Cr_2O_7^{2-}

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(D) When dichromate ion oxidises $Fe^{2+}$ ions in aqueous acidic medium to $Fe^{3+}$,the following balanced redox reaction takes place:$Cr_2O_7^{2-} + 14H^{+} + 6Fe^{2+} \rightarrow 2Cr^{3+} + 6Fe^{3+} + 7H_2O$From the balanced equation,it is clear that $14$ protons ($H^{+}$ ions) are consumed for every $1$ mole of dichromate ion reacting with $6$ moles of $Fe^{2+}$ ions.Therefore,the correct option is $(D)$.

Class 11 Chemistry Redox Reactions Redox reaction and Method for balancing Redox reaction

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How many protons will be consumed when dichromate ion oxidises $Fe^{2+}$ ions in aqueous acidic medium?

TS EAMCET 2019 All TS EAMCET

A
$4$
B
$6$
C
$10$
D
$14$

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Redox Reactions

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Redox reaction and Method for balancing Redox reaction

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How many protons will be consumed when dichromate ion oxidises $Fe^{2+}$ ions in aqueous acidic medium?

Similar Questions

Assign $A, B, C, D$ from the given type of reaction.$NH_4Cl + NaNO_2 \xrightarrow{\Delta} N_2 \uparrow + NaCl + 2H_2O$

The equivalent weight of $Na_2S_2O_3$ (Gram molecular weight $= M$) in the given reaction is $I_2 + 2Na_2S_2O_3 \rightarrow 2NaI + Na_2S_4O_6$.

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$NH_4Cl + NaNO_2 \xrightarrow{\Delta} N_2 \uparrow + NaCl + 2H_2O$

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