How can we know beforehand that free chlorine will form in MnO2+4HCl - MnCl2 +Cl2+2H2O?

Question

MnO2+4HCl -> MnCl2 +Cl2+2H2O

How can we know beforehand that some of the chlorine will break free? Can the reaction happen this way:

MnO2+4HCl ->MnCl4 +2H2O

After all, other oxides react with HCl without a redox reaction, so no free Cl is formed:

CaO + 2HCl = CaCl2 + H2O

Mateo Aguilar · Accepted Answer

In MnO2, Mn is in +4 oxidation state, It has also a lower stable oxidation state +2.but Ca has got only one oxidation state +2.
SO MnO2 acts as oxidizing agent but CaO does not.

Here, Mn(+4) in MnO2 oxidizes the chloride ion to chlorine; Mn+4 will take up the electron from the Cl ion, preventing the production of MnCl4.

Luna Chen · Answer

undefined We can predict that free chlorine will form in the reaction $ \text{MnO}_2 + 4\text{HCl} \rightarrow \text{MnCl}_2 + \text{Cl}_2 + 2\text{H}_2\text{O} $ because manganese dioxide ($ \text{MnO}_2 $) is a strong oxidizing agent, and hydrochloric acid ($ \text{HCl} $) is a source of chloride ions ($ \text{Cl}^- $). In acidic conditions, manganese dioxide oxidizes chloride ions to chlorine gas ($ \text{Cl}_2 $), which is released as a product of the reaction.

How can we know beforehand that free chlorine will form in MnO2+4HCl -&gt; MnCl2 +Cl2+2H2O?

MnO2+4HCl -> MnCl2 +Cl2+2H2O How can we know beforehand that some of the chlorine will break free? Can the reaction happen this way: MnO2+4HCl ->MnCl4 +2H2O After all, other oxides react with HCl without a redox reaction, so no free Cl is formed: CaO + 2HCl = CaCl2 + H2O

How can we know beforehand that free chlorine will form in MnO2+4HCl -> MnCl2 +Cl2+2H2O?

MnO2+4HCl -> MnCl2 +Cl2+2H2O

How can we know beforehand that some of the chlorine will break free? Can the reaction happen this way:

MnO2+4HCl ->MnCl4 +2H2O

After all, other oxides react with HCl without a redox reaction, so no free Cl is formed:

CaO + 2HCl = CaCl2 + H2O