Maharashtra Board Solutions for Chapter: Redox Reactions, Exercise 4: Exercises

Which of the following redox couple is stronger reducing agent ?

$$\begin{gathered} \mathrm{a}. \mathrm{Li} ({\mathrm{E}}^{\circ }=-3.05\mathrm{V}) \mathrm{and} \mathrm{Mg} ({\mathrm{E}}^{\circ }=-2.36\mathrm{V}) \\ \mathrm{b}. \mathrm{Zn} ({\mathrm{E}}^{\circ }=-0.76\mathrm{V}) \mathrm{and} \mathrm{Fe} ({\mathrm{E}}^{\circ }=-0.44\mathrm{V}) \end{gathered}$$

Balance the following reaction by oxidation number method

${\mathrm{Cr}}_2{{\mathrm{O}}_2}^{2⊝}\left(\mathrm{aq}\right) + {{\mathrm{SO}}_3}^{2⊝}\left(\mathrm{aq}\right)\to {\mathrm{Cr}}^{3\oplus }\left(\mathrm{aq}\right)+{{\mathrm{SO}}_4}^{2⊝}\left(\mathrm{aq}\right)\left(\mathrm{acidic}\right)$

Balance the following reaction by oxidation number method in basic medium

${\mathrm{MnO}}_4^{-}\left(\mathrm{aq}\right) + {\mathrm{Br}}^{-}\left(\mathrm{aq}\right) \underset{}{\to } {\mathrm{BrO}}_3^{-}\left(\mathrm{aq}\right) + {\mathrm{MnO}}_2\left(\mathrm{s}\right)$

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Balance the following reaction by oxidation number method in acidic medium:

${\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right) + \mathrm{C}\left(\mathrm{s}\right) \to {\mathrm{CO}}_2\left(\mathrm{g}\right) + {\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Balance the following reaction by oxidation number method(Oxidation no. method)

$\stackrel{}{\mathrm{Bi}(\mathrm{OH}{)}_3}\left(\mathrm{g}\right) + \stackrel{}{\mathrm{Sn}}\left(\mathrm{OH}{{)}_3}^{-}\right(\mathrm{aq}) \underset{}{\to } \mathrm{Bi}(\mathrm{s}) + \stackrel{}{\mathrm{Sn}}(\mathrm{OH}{{)}_6}^{2-}\left(\mathrm{aq}\right)$

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Balance the following redox equation by half reaction method

${\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4 \left(\mathrm{aq}\right) + {{\mathrm{MnO}}_4}^{⊝} \left(\mathrm{aq}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right) + {\mathrm{Mn}}^{2\oplus }\left(\mathrm{aq}\right)\left(\mathrm{acidic}\right)$

Balance the following redox equation by half reaction method

$\mathrm{Bi} (\mathrm{OH}{)}_3 (\mathrm{s}) + {{\mathrm{SnO}}_2}^{2⊝}(\mathrm{aq}) \to {{\mathrm{SnO}}_3}^{2⊝}(\mathrm{aq}) + \mathrm{Bi}(\mathrm{s}\left)\right(\mathrm{basic})$

Complete the following table:

Assign oxidation number to the underlined species and write stock notation of compound

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