A 6.32-g sample of potassium chlorate was decomposed according to the following equation: 2KClO₃ $\rightarrow$ 2KCl + 3O₂
How many moles of oxygen are formed?

Question

A 6.32-g sample of potassium chlorate was decomposed according to the following equation: 2KClO₃ $\rightarrow$ 2KCl + 3O₂ How many moles of oxygen are formed?

Quizplus · Accepted Answer

First, we need to calculate the moles of potassium chlorate using its molar mass.
molar mass of KClO3 = 39.1 + 35.5 + 3(16) = 122.5 g/mol
moles of KClO3 = 6.32 g / 122.5 g/mol = 0.0516 mol

According to the balanced equation, 2 moles of KClO3 produce 3 moles of O2.
So, moles of O2 produced = (3/2) x 0.0516 = 0.0774 mol

Therefore, the correct answer is B.

A 632-G Sample of Potassium Chlorate Was Decomposed According to the the Following