The equations for three reactions involving chlorine or its compounds are listed. $$\[ \begin{array}{ll} 1 & 2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl}+3 \mathrm{O}_{2} \\ 2 & 4 \mathrm{KClO}_{3} \rightarrow 3 \mathrm{KClO}_{4}+\mathrm{KCl} \\ 3 & 6 \mathrm{KOH}+3 \mathrm{Cl}_{2} \rightarrow 3 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{KCl}+\mathrm{KClO}_{3} \end{array} \]$$ Which statement about these equations is correct?

Equation 1 describes the formation of a compound used to kill bacteria in drinking water.

Equation 1 does not represent a redox reaction.

Equation 2 describes the formation of potassium chlorate(IV).

Equations 2 and 3 both represent disproportionation reactions.

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_m24_qp_12 Year：2024 Question No：23

Answer:

Knowledge points:

11.4.1 describe and interpret, in terms of changes in oxidation number, the reaction of chlorine with cold and with hot aqueous sodium hydroxide and recognise these as disproportionation reactions

11.4.2 explain, including by use of an equation, the use of chlorine in water purification to include the production of the active species HOCl and which kill bacteria.

Answer:

Knowledge points:

Solution:

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