Suppose you are provided with a 36.89 g sample of potassium chlorate to perform this experiment. What is the mass of oxygen you expect to release upon heating?

14.45 g of O₂.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2KClO₃ —> 2KCl + 3O₂

Next, we shall determine the mass of KClO₃ that decomposed and the mass of O₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of KClO₃ = 39 + 35.5 + (16×3)

= 39 + 35.5 + 48

= 122.5 g/mol

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

Molar mass of O₂ = 2 ×16 = 32 g/mol

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

SUMMARY:

From the balanced equation above,

245 g of KClO₃ decomposed to produce 96 g of O₂.

Finally, we shall determine the mass of O₂ produced by heating 36.89 g of KClO₃. This can be obtained as follow:

From the balanced equation above,

245 g of KClO₃ decomposed to produce 96 g of O₂.

Therefore, 36.89 g of KClO₃ will decompose to produce =

(36.89 × 96)/245 = 14.45 g of O₂

Thus, 14.45 g of O₂ were obtained from the reaction.

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.

b) nuclear ive learned that in a pedtrodic table