To determine how many moles of [tex]\( KCl \)[/tex] will be formed from 2.73 moles of [tex]\( KClO_3 \)[/tex], we need to look at the balanced chemical equation:
[tex]\[ 2 \, KClO_3 \rightarrow 2 \, KCl + 3 \, O_2 \][/tex]
This equation tells us that 2 moles of [tex]\( KClO_3 \)[/tex] produce 2 moles of [tex]\( KCl \)[/tex].
We can see that the stoichiometric ratio of [tex]\( KClO_3 \)[/tex] to [tex]\( KCl \)[/tex] is 1:1. This means that for every mole of [tex]\( KClO_3 \)[/tex] that reacts, one mole of [tex]\( KCl \)[/tex] is formed.
Since we have 2.73 moles of [tex]\( KClO_3 \)[/tex], it will produce an equivalent amount of [tex]\( KCl \)[/tex]. Hence, 2.73 moles of [tex]\( KClO_3 \)[/tex] will produce 2.73 moles of [tex]\( KCl \)[/tex].
Therefore, the number of moles of [tex]\( KCl \)[/tex] formed is:
[tex]\[ \boxed{2.73} \][/tex]
Thus, the correct answer is [tex]\( 2.73 \)[/tex] moles.
