mathrm(CH)_(3)-mathrm(CH)=mathrm(CH)-mathrm(CH)_(3) mathrm(KMnO)_(4), mathrm(H)_(2) mathrm(O)_(2) mathrm(O)

The given chemical reaction involves the compound \( \mathrm{CH}_{3}-\mathrm{CH}=\mathrm{CH}-\mathrm{CH}_{3} \) (which is 2-butene) reacting with \( \mathrm{KMnO}_{4} \) and \( \mathrm{H}_{2}\mathrm{O}_{2} \) (which is potassium permanganate and hydrogen peroxide, respectively).<br /><br />In this reaction, 2-butene is oxidized to form 1,2-dibromo-2-butene. The reaction proceeds as follows:<br /><br />\[ \mathrm{CH}_{3}-\mathrm{CH}=\mathrm{CH}-\mathrm{CH}_{3} + \mathrm{KMnO}_{4} + \mathrm{H}_{2}\mathrm{O}_{2} \rightarrow \mathrm{CH}_{3}-\mathrm{CHBr}-\mathrm{CHBr}-\mathrm{CH}_{3} + \mathrm{MnO}_{2} + \mathrm{KOH} \]<br /><br />Here, \( \mathrm{KMnO}_{4} \) and \( \mathrm{H}_{2}\mathrm{O}_{2} \) act as oxidizing agents, leading to the addition of bromine across the double bond in 2-butene. The product formed is 1,2-dibromo-2-butene, where the double bond is replaced by two bromine atoms.<br /><br />The balanced chemical equation for this reaction is:<br /><br />\[ \mathrm{CH}_{3}-\mathrm{CH}=\mathrm{CH}-\mathrm{CH}_{3} + \mathrm{KMnO}_{4} + \mathrm{H}_{2}\mathrm{O}_{2} \rightarrow \mathrm{CH}_{3}-\mathrm{CHBr}-\mathrm{CHBr}-\mathrm{CH}_{3} + \mathrm{MnO}_{2} + \mathrm{KOH} \]<br /><br />This reaction is an example of an oxidation reaction where the double bond in 2-butene is broken and replaced by two bromine atoms, forming 1,2-dibromo-2-butene.