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 25 °c and a pressure of 749 mm hg. if the wet o2 gas formed occupies a volume of 5.76 l, the number of moles of kclo3 reacted was mol. the vapor pressure of water is 23.8 mm hg at 25 °c.

The number of moles of KClO₃ reacted was 0,15 mol

Explanation:

For the reaction:

2KClO₃(s) → 2KCl(s) + 2O₂(g)

The only gas product is O₂.

Total pressure is the sum of vapor pressure of water with O₂ gas formed. Thus, pressure of O₂ is:

749mmHg - 23,8mmHg = 725,2mmHg

Using gas law:

PV/RT = n

Where:

P is pressure (725,2mmHg ≡ 0,9542atm)

V is volume (5,76L)

R is gas constant (0,082 atmL/molK)

And T is temperature (25°C ≡ 298,15K)

Replacing, number of moles of O₂ are 0,2248 moles

As 2 moles of KClO₃ react with 3 moles of O₂ the moles of KClO₃ that reacted was:

0,2248 mol O₂× = 0,15 mol of KClO₃

I hope it helps!