Oxygen gas can be prepared by heating potassium chlorate according to the following equation:

2KClO3(s) → 2KCl(s) + 3O2(g)

The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 747 mm Hg. If the wet O2 gas formed occupies a volume of 6.42 L, the number of grams of O2 formed is g. The vapor pressure of water is 17.5 mm Hg at 20 °C.

The number of grams of formed is 8.32 g

Explanation:

According to the ideal gas equation:

P = Pressure of the gas = Total pressure - presure of water = (747-17.5)mm Hg= 729.5 mm Hg = 0.96 atm     (760mmHg=1atm)

V= Volume of the gas = 6.42 L

n=  moles of gas = ?

T= Temperature of the gas in kelvin =

R= Gas constant = 0.0821Latm/Kmol

The balanced chemical reaction is:

Mass of produced=

Thus number of grams of formed is 8.32 g

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