Final answer:
The pressure exerted by 32 g of O₂ in a 22.0 L container at 30.0 °C is approximately 0.945 atm.
Step-by-step explanation:
To calculate the pressure exerted by 32 g of O₂ in a 22.0 L container at 30.0 °C, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the mass of O₂ to moles using its molar mass. The molar mass of O₂ is 32 g/mol, so the number of moles of O₂ is 32 g ÷ 32 g/mol = 1 mol.
Next, we can substitute the known values into the ideal gas law equation:
(P)(22.0 L) = (1 mol)(0.0821 L·atm/mol·K)(30.0 °C + 273.15) K.
Solving for P, we find that the pressure exerted by 32 g of O₂ in a 22.0 L container at 30.0 °C is approximately 0.945 atm.