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MnO(2) + 4 HCI rarr MnCI(2) + 2H(2)O + C...

`MnO_(2) + 4 HCI rarr MnCI_(2) + 2H_(2)O + CI_(2)`.
Identify the substance oxidized in the above equation.

A

`MnCI_(2)`

B

HCI

C

`H_(2)O`

D

`NbO_(2)`

Text Solution

AI Generated Solution

The correct Answer is:
To identify the substance oxidized in the given reaction, we need to analyze the oxidation states of the elements involved before and after the reaction. The reaction is: \[ \text{MnO}_2 + 4 \text{HCl} \rightarrow \text{MnCl}_2 + 2 \text{H}_2\text{O} + \text{Cl}_2 \] ### Step 1: Assign oxidation states We will assign oxidation states to each element in the reaction. - In \(\text{MnO}_2\): - Oxygen (O) has an oxidation state of -2. - Let the oxidation state of Manganese (Mn) be \(x\). - The equation becomes: \(x + 2(-2) = 0 \Rightarrow x - 4 = 0 \Rightarrow x = +4\). - Thus, Mn in \(\text{MnO}_2\) has an oxidation state of +4. - In \(\text{HCl}\): - Hydrogen (H) has an oxidation state of +1. - Chlorine (Cl) has an oxidation state of -1. - In \(\text{MnCl}_2\): - Let the oxidation state of Mn be \(y\). - The equation becomes: \(y + 2(-1) = 0 \Rightarrow y - 2 = 0 \Rightarrow y = +2\). - Thus, Mn in \(\text{MnCl}_2\) has an oxidation state of +2. - In \(\text{H}_2\text{O}\): - Hydrogen (H) has an oxidation state of +1. - Oxygen (O) has an oxidation state of -2. - In \(\text{Cl}_2\): - Chlorine (Cl) in its elemental form has an oxidation state of 0. ### Step 2: Compare oxidation states before and after the reaction Now we will compare the oxidation states of Mn and Cl before and after the reaction: - **Manganese (Mn)**: - In \(\text{MnO}_2\): +4 - In \(\text{MnCl}_2\): +2 - **Change**: +4 to +2 (reduction) - **Chlorine (Cl)**: - In \(\text{HCl}\): -1 - In \(\text{Cl}_2\): 0 - **Change**: -1 to 0 (oxidation) ### Conclusion From the analysis, we can conclude that: - Manganese is reduced (its oxidation state decreases from +4 to +2). - Chlorine is oxidized (its oxidation state increases from -1 to 0). Therefore, the substance that is oxidized in the reaction is **Chlorine (Cl)**.
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