Which compound is formed when $H_2S$ gas is passed through an acidic solution of $KMnO_4$?
- A$K_2S$
- B$S$
- C$K_2SO_3$
- D$MnO_2$
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Similar Questions
What is the value of $x$ in order to balance the following redox reaction by the ion-electron method?
$x H_2O_2 + ClO_4^{-} \rightarrow x O_2 + ClO_2^{-} + 2 H_2O$
$x H_2O_2 + ClO_4^{-} \rightarrow x O_2 + ClO_2^{-} + 2 H_2O$
When $SO_{2}$ is passed through acidified $K_{2}Cr_{2}O_{7}$,the process that takes place is
$aIO_3^- + bI^- + 6H^+ \to cI_2 + 3H_2O$
In the above reaction,the coefficients $a$,$b$,and $c$ are respectively:
In the above reaction,the coefficients $a$,$b$,and $c$ are respectively:
Medium
View SolutionThe number of moles of $KMnO_4$ that will be needed to react completely with one mole of ferrous oxalate $FeC_2O_4$ in acidic solution is
What is the ratio of the stoichiometric coefficient of $N_2H_4$ to $Cl^-$ in the following balanced redox reaction?
$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$
$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$
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