Mass of O₂ formed = 7.84 g
Further explanation
Given
Reaction
2KClO₃(s) ⇒2KCl(s) + 3O₂(g)
P water = 23.8 mmHg
P tot = 755 mmHg
V = 6.22 L
T = 25 + 273 = 298 K
Required
mass of O₂
Solution
P tot = P O₂ + P water
P O₂ = P tot - P water
P O₂ = 755 - 23.8
P O₂ = 731.2mmHg = 0.962 atm
Ideal gas law :
n = PV/RT
n = 0.962 x 6.22 / 0.082 x 298
n = 0.245
= mol x MW
= 0.245 x 32
= 7.84 g