(C) The reaction is: $2NaNO_2 + 3FeSO_4 + 3H_2SO_4 \longrightarrow Fe_2(SO_4)_3 + Na_2SO_4 + 2H_2O + 2NO$Then,$FeSO_4 + NO + 5H_2O \longrightarrow [Fe

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$C$. Intermolecular redox reaction.

(C) The reaction is: $2NaNO_2 + 3FeSO_4 + 3H_2SO_4 \longrightarrow Fe_2(SO_4)_3 + Na_2SO_4 + 2H_2O + 2NO$Then,$FeSO_4 + NO + 5H_2O \longrightarrow [Fe(H_2O)_5NO]SO_4$.In the first step,the oxidation state of $N$ changes from $+3$ (in $NaNO_2$) to $+2$ (in $NO$),and the oxidation state of $Fe$ changes from $+2$ (in $FeSO_4$) to $+3$ (in $Fe_2(SO_4)_3$).Since different elements are oxidized and reduced in the same reaction,it is an intermolecular redox reaction.

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

Medium

Assign $A, B, C, D$ from the given type of reaction.
$NaNO_2 + FeSO_4 + H_2SO_4 \longrightarrow [Fe(H_2O)_5NO]SO_4 + Na_2SO_4 + Fe_2(SO_4)_3 + H_2O$
Identify the type of reaction for the formation of the brown ring complex.

A
$A$. Disproportionation reaction.
B
$B$. Comproportionation reaction.
C
$C$. Intermolecular redox reaction.
D
$D$. Thermal decomposition redox reaction.

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Class 11

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Redox Reactions

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Redox reaction and Method for balancing Redox reaction

Justify that the reaction:
$2 Cu_{2}O_{(s)} + Cu_{2}S_{(s)} \rightarrow 6 Cu_{(s)} + SO_{2(g)}$
is a redox reaction. Identify the species oxidised/reduced,which acts as an oxidant and which acts as a reductant.

Medium

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For the given redox reaction: $a MnO_4^{-} + b S_2 O_3^{2-} + H_2 O \longrightarrow x MnO_2 + y SO_4^{2-} + z OH^-$,the values of $a$ and $y$ respectively are:

MediumKCET 2023

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In the reaction between $KI$ and acidic potassium dichromate solution,the oxidation state of chromium in the final product is ........

Medium

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$MnO_4^{-}$ oxidises $(i)$ oxalate ion in acidic medium at $333 \ K$ and $(ii)$ $HCl$. For balanced chemical equations,the ratios $[MnO_4^{-} : C_2O_4^{2-}]$ in $(i)$ and $[MnO_4^{-} : HCl]$ in $(ii)$ respectively are

MediumKVPY 2011

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Molecular weight of $Cu_2S$ is $M$. In the following reaction its equivalent weight is $M / x$. What is $x$?
$Cu_2S + MnO_4^{-} \rightarrow Cu^{2+} + Mn^{2+} + SO_2$

Medium

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Assign $A, B, C, D$ from the given type of reaction.$NaNO_2 + FeSO_4 + H_2SO_4 \longrightarrow [Fe(H_2O)_5NO]SO_4 + Na_2SO_4 + Fe_2(SO_4)_3 + H_2O$Identify the type of reaction for the formation of the brown ring complex.

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Justify that the reaction:$2 Cu_{2}O_{(s)} + Cu_{2}S_{(s)} \rightarrow 6 Cu_{(s)} + SO_{2(g)}$is a redox reaction. Identify the species oxidised/reduced,which acts as an oxidant and which acts as a reductant.

For the given redox reaction: $a MnO_4^{-} + b S_2 O_3^{2-} + H_2 O \longrightarrow x MnO_2 + y SO_4^{2-} + z OH^-$,the values of $a$ and $y$ respectively are:

In the reaction between $KI$ and acidic potassium dichromate solution,the oxidation state of chromium in the final product is ........

$MnO_4^{-}$ oxidises $(i)$ oxalate ion in acidic medium at $333 \ K$ and $(ii)$ $HCl$. For balanced chemical equations,the ratios $[MnO_4^{-} : C_2O_4^{2-}]$ in $(i)$ and $[MnO_4^{-} : HCl]$ in $(ii)$ respectively are

Molecular weight of $Cu_2S$ is $M$. In the following reaction its equivalent weight is $M / x$. What is $x$?$Cu_2S + MnO_4^{-} \rightarrow Cu^{2+} + Mn^{2+} + SO_2$

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Assign $A, B, C, D$ from the given type of reaction.
$NaNO_2 + FeSO_4 + H_2SO_4 \longrightarrow [Fe(H_2O)_5NO]SO_4 + Na_2SO_4 + Fe_2(SO_4)_3 + H_2O$
Identify the type of reaction for the formation of the brown ring complex.

Justify that the reaction:
$2 Cu_{2}O_{(s)} + Cu_{2}S_{(s)} \rightarrow 6 Cu_{(s)} + SO_{2(g)}$
is a redox reaction. Identify the species oxidised/reduced,which acts as an oxidant and which acts as a reductant.

Molecular weight of $Cu_2S$ is $M$. In the following reaction its equivalent weight is $M / x$. What is $x$?
$Cu_2S + MnO_4^{-} \rightarrow Cu^{2+} + Mn^{2+} + SO_2$