Determine the mass of oxygen produced in the decomposition of 25.0 g of potassium
chlorate, which would also yield the formation of potassium chloride. Show steps please!

9.80g of O2.

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

2KClO3 —> 2KCl + 3O2

Step 2:

Determination of the mass of KClO3 that decomposed and the mass of O2 produced from the balanced equation. This is illustrated below:

Molar Mass of KClO3 = 39 + 35.5 + (16x3) = 122.5g/mol

Mass of KClO3 from the balanced equation = 2 x 122.5 = 245g

Molar Mass of O2 = 16x2 = 32g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96g.

From the balanced equation above, 245g of KClO3 decomposed to produce 96g of O2.

Step 3:

Determination of the mass of O2 produced in the decomposition of 25.0g of KClO3. This is illustrated below:

From the balanced equation above, 245g of KClO3 decomposed to produce 96g of O2.

Therefore, 25g of KClO3 will decompose to produce = (25x96)/245 =

9.80g of O2.

Therefore, 9.80g of O2 is produced from the decomposition of 25g of KClO3.

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