In the following reaction,$\text{SO}_2 + 2\text{H}_2\text{S} \to 3\text{S} + 2\text{H}_2\text{O}$,which choice has a value twice that of the equivalent mass of the oxidising agent?
- A$64$
- B$32$
- C$16$
- D$48$
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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$NaH_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(aq)} + H_{2(g)} \uparrow$
$NaH_{(s)} + H_2O_{(l)} \longrightarrow NaOH_{(aq)} + H_{2(g)} \uparrow$
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View Solution$A$ given amount of $Fe^{2+}$ is oxidized by $x \ mol$ of $MnO_{4}^{-}$ in acidic medium. The number of moles of $Cr_{2}O_{7}^{2-}$ required to oxidize the same amount of $Fe^{2+}$ in acidic medium is
MediumWBJEE 2021
View SolutionHow many electrons $(e^-)$ are gained by the oxidizing agent $KMnO_4$ to convert into $MnO_4^{2-}$,$MnO_2$,$Mn_2O_3$,and $Mn^{2+}$ respectively?
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View Solution$Cu^{2+}(aq.)$ does not undergo a redox reaction with a solution of:
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View SolutionMatch List-$I$ with the List-$II$.
List-$I$ (Reaction) List-$II$ (Type of redox reaction) $A$. $N_{2(g)} + O_{2(g)} \rightarrow 2 NO_{(g)}$ $I$. Decomposition $B$. $2 Pb(NO_3)_{2(s)} \rightarrow 2 PbO_{(s)} + 4 NO_{2(g)} + O_{2(g)}$ $II$. Displacement $C$. $2 Na_{(s)} + 2 H_2 O_{(l)} \rightarrow 2 NaOH_{(aq)} + H_{2(g)}$ $III$. Disproportionation $D$. $2 NO_{2(g)} + 2 OH^-_{(aq)} \rightarrow NO^-_{2(aq)} + NO^-_{3(aq)} + H_2 O_{(l)}$ $IV$. Combination
Choose the correct answer from the options given below:
| List-$I$ (Reaction) | List-$II$ (Type of redox reaction) |
| $A$. $N_{2(g)} + O_{2(g)} \rightarrow 2 NO_{(g)}$ | $I$. Decomposition |
| $B$. $2 Pb(NO_3)_{2(s)} \rightarrow 2 PbO_{(s)} + 4 NO_{2(g)} + O_{2(g)}$ | $II$. Displacement |
| $C$. $2 Na_{(s)} + 2 H_2 O_{(l)} \rightarrow 2 NaOH_{(aq)} + H_{2(g)}$ | $III$. Disproportionation |
| $D$. $2 NO_{2(g)} + 2 OH^-_{(aq)} \rightarrow NO^-_{2(aq)} + NO^-_{3(aq)} + H_2 O_{(l)}$ | $IV$. Combination |
Choose the correct answer from the options given below:
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