How many protons will be consumed when dichro | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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-}

Vedclass · Accepted Answer

$14$

Vedclass · Answer

(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 $(D)$.

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

Similar Questions

The product of oxidation of $I^-$ ion by $MnO_4^-$ in alkaline medium is

In the equation $H_2S + 2HNO_3 \to 2H_2O + 2NO_2 + S$,the equivalent weight of hydrogen sulphide is:

$2MnO_4^{-} + 5H_2O_2 + 6H^{+} \to 2Z + 5O_2 + 8H_2O$. In this reaction $Z$ is

Observe the following reaction: $I_2 + 10 HNO_3 \rightarrow 2 HIO_3 + 10 NO_2 + 4 H_2O$. The equivalent weight of $HNO_3$ is (molar mass of $HNO_3 = M$).

For the following balanced equation,$a, b, c$ and $d$ will be respectively:
$IO_3^- + aI^- + bH^+ \to cH_2O + dI_2$

Vedclass Test Series

Exam Paper Generator

Online Exam Module