Question

Oxygen gas generated in the thermal decomposition of potassium chlorate is collected over water. The volume of gas collected is 0.128 L, at a temperature of 297K and a pressure of 762 mm Hg. The vapour pressure of H2O at 297K is 22.4 torr. What is the mass of oxygen collected?

Answer 1

The mass of oxygen collected from the thermal decomposition of potassium chlorate at a temperature of 297 K and 762 mmHg is 0.16 g

How to determine the mole of oxygen produced

We'll begin by obtaining the number of mole of oxygen gas produced from the reaction. This can be obtained by using the ideal gas equation as illustrated below:

• Volume (V) = 0.128 L
• Temperature (T) = 297 K
• Pressure (P) = 762 – 22.4 = 739.6 mmHg
• Gas constant (R) = 62.363 mmHg.L/Kmol
• Number of mole (n) =?

PV = nRT

739.6 × 0.128 = n × 62.363 × 297

Divide both sides by 62.363 × 297

n = (739.6 × 0.128) / (62.363 × 297)

n = 0.0051 mole

Thus, the number of mole of oxygen gas produced is 0.0051 mole

How to determine the mass of oxygen collected

Haven obtain the number of mole of oxygen gas produced, we can determine the mass of the oxygen produced as follow:'

• Mole = 0.0051 mole
• Molar mass of oxygen gas = 32 g/mole
• Mass of oxygen =?

Mole = mass / molar mass

0.0051 = mass of oxygen / 32

Cross multiply

Mass of oxygen = 0.0051 × 32

Mass of oxygen = 0.16 g

Thus, we can conclude that the mass of oxygen gas collected is 0.16 g

Learn more about ideal gas equation:

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