Final answer:
To find the volume occupied by 22.1 g of O₂ at 52°C and 1.63 atm, we can use the Ideal Gas Law equation. First, we convert the mass of O₂ to moles, then we calculate the volume using the equation (nRT) / P. The volume is approximately 12.63 liters.
Step-by-step explanation:
To solve this problem, we can use the Ideal Gas Law equation, which states that PV = nRT. In this equation, 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. We can rearrange the equation to solve for the volume:
V = (nRT) / P
Given the values in the question, we have:
Mass of O₂ : 22.1 g
Pressure: 1.63 atm
Temperature: 52°C = 325 K
First, we need to convert the mass of O2 to moles. The molar mass of O₂ is 32 g/mol, so:
n = mass / molar mass = 22.1 g / 32 g/mol = 0.69 mol
Now, we can calculate the volume:
V = (nRT) / P = (0.69 mol)(0.0821 L·atm/(mol·K))(325 K) / 1.63 atm ≈ 12.63 L
Therefore, the volume occupied by 22.1 g of O₂ at 52°C and a pressure of 1.63 atm is approximately 12.63 liters.