Question

The equation represents the breakdown of potassium chlorate (KClO3)

2KClO3 --> 2KCl + 3O2

How many moles of oxygen can be produced from 0.16 moles of potassium chlorate?

Responses

0.24 mol
0.24 mol

0.48 mol
0.48 mol

0.34 mol
0.34 mol

0.11 mol

Answer 1

To determine how many moles of oxygen (\(O_2\)) can be produced from a given amount of potassium chlorate (\(KClO_3\)), we can use the stoichiometry of the balanced chemical equation:

\[
2KClO_3 \rightarrow 2KCl + 3O_2
\]

From the equation, we see that 2 moles of \(KClO_3\) produce 3 moles of \(O_2\).

We can set up the stoichiometric ratios:

- From 2 moles of \(KClO_3\) → 3 moles of \(O_2\)

To find out how many moles of \(O_2\) are produced from 0.16 moles of \(KClO_3\), we can use the ratio:

\[
\text{Moles of } O_2 = 0.16 \, \text{moles of } KClO_3 \times \left(\frac{3 \, \text{moles of } O_2}{2 \, \text{moles of } KClO_3}\right)
\]

Calculating this gives:

\[
\text{Moles of } O_2 = 0.16 \times \frac{3}{2} = 0.16 \times 1.5 = 0.24 \, \text{moles of } O_2
\]

Therefore, from 0.16 moles of potassium chlorate, you can produce **0.24 moles of oxygen**.

The correct response is:

**0.24 mol**