Moles of K_2Cr_2O_7 used to oxidise 1 mole of | vedclass

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

Question

(C) In $Fe_{0.92}O$,let the oxidation state of $Fe$ be $x$. Since the oxidation state of $O$ is $-2$,we have $0.92x + (-2) = 0$,so $x = \frac{2}{0.92}

Vedclass · Accepted Answer

$\frac{0.76}{6}$

Vedclass · Answer

(C) In $Fe_{0.92}O$,let the oxidation state of $Fe$ be $x$. Since the oxidation state of $O$ is $-2$,we have $0.92x + (-2) = 0$,so $x = \frac{2}{0.92}$.When $1$ $mole$ of $Fe_{0.92}O$ is oxidized to $Fe^{3+}$,the change in oxidation state of $Fe$ is $(3 - \frac{2}{0.92}) 	imes 0.92 = 3 	imes 0.92 - 2 = 2.76 - 2 = 0.76$.$K_2Cr_2O_7$ acts as an oxidizing agent where $Cr$ changes from $+6$ to $+3$,a change of $3$ per $Cr$ atom,or $6$ per $K_2Cr_2O_7$ molecule.Equating the total change in oxidation states: $n 	imes 6 = 0.76$.Therefore,$n = \frac{0.76}{6}$ $moles$.

Moles of $K_2Cr_2O_7$ used to oxidise $1$ $mole$ of $Fe_{0.92}O$ to $Fe^{3+}$ are -

Similar Questions

Fluorine reacts with ice and results in the change:
$H_2O_{(s)} + F_{2(g)} \rightarrow HF_{(g)} + HOF_{(g)}$
Justify that this reaction is a redox reaction.

Assign $A, B, C, D$ from the given type of reaction.
$MnO_2 + 2KOH + \frac{1}{2}O_2 \longrightarrow K_2MnO_4 + H_2O$

$H^{+} + Cr_2O_7^{2-} + SO_3^{2-} \to Cr^{3+} + SO_4^{2-} + H_2O$. In the balanced reaction,the coefficients of $H^{+}$ and $SO_4^{2-}$ will be respectively:

Which of the following reagents causes the aqueous colored solution of acidic $KMnO_4$ to become colorless?

Calculate the equivalent weight of $KMnO_4$ in acidic,basic,and neutral media.

Vedclass Test Series

Exam Paper Generator

Online Exam Module