CUET Preparation Today
In the reaction below, identify the species undergoing oxidation and reduction. $ \text{H}_2\text{S}(\text{g})+\text{Cl}_2(\text{g})\rightarrow2\text{HCl}(\text{g})+\text{S}(\text{s}) $ |
$H_2S$ is oxidized and $Cl_2$ is reduced $H_2S$ and $Cl_2$ both are reduced $Cl_2$ and $H_2S$ both are oxidized $H_2S$ is reduced and $Cl_2$ is oxidized |
$H_2S$ is oxidized and $Cl_2$ is reduced |
The correct answer is Option (1) → $H_2S$ is oxidized and $Cl_2$ is reduced In $H_2S$: Sulfur is in the –2 oxidation state. In product S (elemental sulfur): Oxidation state = 0 Therefore there is increase in oxidation state → oxidation. In $Cl_2$: Chlorine is in the 0-oxidation state. In $HCl$: Chlorine is in the –1 oxidation state Therefore there is decrease in oxidation state → reduction. $H_2S$ is oxidized and $Cl_2$ is reduced. |
