Assign $A, B, C, D$ from the given type of reaction.
$Mg_{(s)} + 2H_2O_{(l)} \xrightarrow{\text{Warm}} Mg(OH)_{2(aq)} + H_{2(g)} \uparrow$
$Mg_{(s)} + 2H_2O_{(l)} \xrightarrow{\text{Warm}} Mg(OH)_{2(aq)} + H_{2(g)} \uparrow$
- Afor disproportionation reaction.
- Bfor comproportionation reaction.
- Cfor either intermolecular redox reaction or displacement reaction.
- Dfor either thermal combination redox reaction or thermal decomposition redox reaction.
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Similar Questions
In alkaline condition $KMnO_4$ reacts as follows:
$2KMnO_4 + 2KOH \to 2K_2MnO_4 + H_2O + O$
Therefore,its equivalent weight will be:
$2KMnO_4 + 2KOH \to 2K_2MnO_4 + H_2O + O$
Therefore,its equivalent weight will be:
Medium
View SolutionBalance the following ionic equations:
$1. Cr_{2}O_{7}^{2-} + H^{+} + I^{-} \to Cr^{3+} + I_{2} + H_{2}O$
$2. Cr_{2}O_{7}^{2-} + Fe^{2+} + H^{+} \to Cr^{3+} + Fe^{3+} + H_{2}O$
$3. MnO_{4}^{-} + SO_{3}^{2-} + H^{+} \to Mn^{2+} + SO_{4}^{2-} + H_{2}O$
$4. MnO_{4}^{-} + H^{+} + Br^{-} \to Mn^{2+} + Br_{2} + H_{2}O$
$1. Cr_{2}O_{7}^{2-} + H^{+} + I^{-} \to Cr^{3+} + I_{2} + H_{2}O$
$2. Cr_{2}O_{7}^{2-} + Fe^{2+} + H^{+} \to Cr^{3+} + Fe^{3+} + H_{2}O$
$3. MnO_{4}^{-} + SO_{3}^{2-} + H^{+} \to Mn^{2+} + SO_{4}^{2-} + H_{2}O$
$4. MnO_{4}^{-} + H^{+} + Br^{-} \to Mn^{2+} + Br_{2} + H_{2}O$
Difficult
View Solution$5H_2O_2 + XClO_2 + 2OH^- \to XCl^- + YO_2 + 6H_2O$
In the above balanced reaction,the reaction is balanced when,
In the above balanced reaction,the reaction is balanced when,
Medium
View SolutionIn an alkaline solution,$ClO_2$ oxidizes $H_2O_2$ to $O_2$ and is itself reduced to $Cl^-$. How many moles of $H_2O_2$ will be oxidized by $1 \ mol$ of $ClO_2$?
Difficult
View SolutionNumber of moles of $K_2Cr_2O_7$ reduced by one mole of $Sn^{2+}$ ions is
Medium
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