JEE Main Redox Reactions Practice Questions With Solutions

Thiosulphate reacts differently with iodine and bromine in the reactions given below:

$\begin{array}{rl}& 2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+{\mathrm{I}}_2\to {\mathrm{S}}_4{\mathrm{O}}_6^{2-}+2{\mathrm{I}}^{-}\\ & {\mathrm{S}}_2{\mathrm{O}}_3^{2-}+5{\mathrm{Br}}_2+5{\mathrm{H}}_2\mathrm{O}\to 2{\mathrm{SO}}_4^{2-}+4{\mathrm{Br}}^{-}+10{\mathrm{H}}^{+}\end{array}$& 2 \left(\textrm{ } S\right)_{2} O_{3}^{2 -} + I_{2} \rightarrow S_{4} O_{6}^{2 -} + 2 I^{-} \\ & S_{2} O_{3}^{2 -} + 5 Br_{2} + 5 H_{2} O \rightarrow 2 SO_{4}^{2 -} + 4 Br^{-} + 10 H^{+}

Which of the following statement justifies the above dual behaviour of thiosulphate?

The number of ions from the following that are expected to behave as oxidising agent is :

${\mathrm{Sn}}^{4+},{\mathrm{Sn}}^{2+},{\mathrm{Pb}}^{2+},{\mathrm{Tl}}^{3+},{\mathrm{Pb}}^{4+},{\mathrm{Tl}}^{+}$Sn^{4 +} , Sn^{2 +} , Pb^{2 +} , Tl^{3 +} , Pb^{4 +} , Tl^{+}

Match List I with List II.

Choose the correct answer from the options given below :

When ${\mathrm{MnO}}_2$MnO_{2} and ${\mathrm{H}}_2{\mathrm{SO}}_4$H_{2} SO_{4} is added to a salt $(\mathrm{A})$\left(\right. A \left.\right), the greenish yellow gas liberated as salt (A) is :

Chlorine undergoes disproportionation in alkaline medium as shown below :

${\mathrm{aCl}}_{2(\mathrm{g})}+\mathrm{b}{\mathrm{OH}}_{(\mathrm{aq})}^{-}\to \mathrm{c}{\mathrm{ClO}}_{(\mathrm{aq})}^{-}+\mathrm{d}{\mathrm{Cl}}_{(\mathrm{aq})}^{-}+\mathrm{e}{\mathrm{H}}_2{\mathrm{O}}_{(\mathrm{l})}$aCl_{2 \left(\right. \textrm{ } g \left.\right)} + b OH_{\left(\right. aq \left.\right)}^{-} \rightarrow c ClO_{\left(\right. aq \left.\right)}^{-} + d Cl_{\left(\right. aq \left.\right)}^{-} + e H_{2} O_{\left(\right. l \left.\right)}

The values of $a,b,c$a , b , c and $d$d in a balanced redox reaction are respectively :

In alkaline medium, ${\mathrm{MnO}}_4^{-}$MnO_{4}^{-} oxidises ${\mathrm{I}}^{-}$I^{-} to

Which of the following cannot function as an oxidising agent?

Given below are two statements:

Statement I : In redox titration, the indicators used are sensitive to change in $\mathrm{pH}$pH of the solution.

Statement II : In acid-base titration, the indicators used are sensitive to change in oxidation potential.

In the light of the above statements, choose the most appropriate answer from the options given below