The reaction Cl(2)(g)+20H^(-)(aq)toClO^(...

The reaction `Cl_(2)(g)+20H^(-)(aq)toClO^(-)(aq)+Cl^(-)(aq)+H_(2)O(l)` represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action.

Text Solution

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`overset(0)(Cl_(2))(g)+2overset(-2)(O)overset(+1)(H^(-))(aq)to overset(+1)(Cl)overset(-2)(O^(-))(aq)+overset(-1)(Cl^(-))(aq)+overset(+1)(H_(2))overset(-2)(O)(l)`
In this reaction, O.N. of Cl increases from 0 ( in `Cl_(2)`) to 1 (in `ClO^(-)`) as well as decreases from 0 (in `Cl_(2)`) to -1 (in `Cl^(-1)`). So, it acts both reducing as well as oxidising agent. This is an example of disproportionation reaction. In this reaction, `ClO^(-)` species bleaches the substances due to its oxidising action. [In hypochlorite ion `(ClO^(-))Cl` can decrease its oxidation number from +1 to 0 or -1.]

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6 L HCl (aq) is consumed for every 3 L `H_2` produced

33.6 L `H_2(g)` is produced regardless temperature and pressure for every moles that reacts .

67.2 L `H_2(g)` at 1 atm , 273 K is produced for every mole Al that reacts .

11.2 L `H_2`(g) at 1 atm, 273 K is produced for every mole HCl(aq) consumed

The reaction, 2H_(2)O(l) to 4H^(+)(aq.)+O_(2)(g)+4^(-) is

a redox reaction

a hydrolysis reaction

a solvolysis reaction

an oscillatory reaction

The reaction Cl_(2(g)) + 2 I_((aq))^(-) to 2 Cl_((aq))^(-) + I_(2(s)) In this anode reaction is -

`Cl_(2) + 2e^(-) to 2 Cl^(-)`

`2I^(-) to I_(2) + 2e^(-)`

`2 Cl^(-) to Cl_(2) + 2e^(-)`

`I_(2) + 2e^(-) to 2I^(-)`