Question

When 86.5 g of calcium chlorate decomposes into calcium chloride and oxygen, how many grams of oxygen are produced? Ca(ClO3)2 → CaCl2 + O2

Answer 1

Answer:

40.1 g

Explanation:

The balanced equation is:

• Ca(ClO₃)₂ → CaCl₂ + 3O₂

First we convert 86.5 g of calcium chlorate into moles, using its molar mass:

• 86.5 g Ca(ClO₃)₂ ÷ 206.98 g/mol = 0.418 mol Ca(ClO₃)₂

Then we convert Ca(ClO₃)₂ moles into O₂ moles, using the stoichiometric coefficients of the balanced reaction:

• 0.418 mol Ca(ClO₃)₂ * $\frac{3molO_2}{1molCa(ClO_3)_2}$ = 1.254 mol O₂

Finally we convert O₂ moles into grams:

• 1.25 mol O₂ * 32 g/mol = 40.1 g O₂