Question

Question #6584b

Answer 1

`"4 moles KClO"_3`

Explanation:

The key here is the balanced chemical equation that describes this decomposition reaction

`2"KClO"_ (3(s)) stackrel(color(white)(acolor(red)(Delta)aaa))(-> ) 2"KCl"_ ((s)) + 3"O"_ (2(g))`

Take a look at the coefficients added to the chemical species that take part in the reaction.

In this case, you know that for every `2` moles of potassium chlorate that undergo decomposition, you get `2` moles of potassium chloride and `3` moles of oxygen gas.

• `2"KClO"_3 -> "2 moles of KClO"_3`
• `"2KCl " -> " 2 moles KCl"`
• `3"O"_2 -> "3 moles O"_2`

This means that in order for the reaction to produce `6` moles of oxygen gas, you need to have

`6 color(red)(cancel(color(black)("moles O"_2))) * overbrace( "2 moles KClO"_3/(3color(red)(cancel(color(black)("moles O"_2)))))^(color(blue)("given by the balanced chemical equation")) = color(darkgreen)(ul(color(black)("4 moles KClO"_3)))`