Final answer:
To find the partial pressure of oxygen gas, we need to determine its mole fraction using the number of moles of oxygen and the total number of moles of gas in the system. The correct answer is b) 388.9 torr.
Step-by-step explanation:
According to the given balanced equation, 2KClO₃(s) -> 2KCl(s) + 3O₂(g), we can see that for every 2 moles of KClO₃, we will produce 3 moles of O₂ gas. Therefore, the mole ratio of O₂ to KClO₃ is 3:2.
To find the partial pressure of O₂, we need to determine its mole fraction. The total number of moles of gas in the system can be calculated using the ideal gas law equation:
PV = nRT
Where P is the total pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
To calculate the partial pressure of O₂, we can use the mole fraction:
X(O₂) = n(O₂) / n(total)
Where X(O₂) is the mole fraction of O₂, n(O₂) is the number of moles of O₂, and n(total) is the total number of moles of gas in the system.
Since we know the mole ratio of O₂ to KClO₃ is 3:2, we can calculate the number of moles of O₂ produced. Then, we can use the total pressure and mole fraction to find the partial pressure of O₂.
The correct answer should be b) 388.9 torr.