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!

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .