1. Determine the Molar Mass of SO₂
* Sulfur (S) has a molar mass of 32.06 g/mol
* Oxygen (O) has a molar mass of 16.00 g/mol
* SO₂ has a molar mass of 32.06 + (16.00 x 2) = 64.06 g/mol
2. Calculate the Number of Moles of SO₂
* Moles = mass / molar mass
* Moles = 72.0 g / 64.06 g/mol
* Moles ≈ 1.124 mol
3. Apply the Ideal Gas Law
* The Ideal Gas Law is PV = nRT, where:
* P = Pressure (in atmospheres)
* V = Volume (in liters)
* n = Number of moles
* R = Ideal Gas Constant (0.0821 L·atm/mol·K)
* T = Temperature (in Kelvin)
4. You Need More Information
To calculate the volume, we need to know the pressure and temperature of the sulfur dioxide gas.
Example:
Let's assume the sulfur dioxide is at standard temperature and pressure (STP):
* T = 273.15 K
* P = 1 atm
Now we can solve for V:
* V = (nRT) / P
* V = (1.124 mol * 0.0821 L·atm/mol·K * 273.15 K) / 1 atm
* V ≈ 25.4 L
Therefore, the volume of 72.0 grams of sulfur dioxide at STP is approximately 25.4 liters.
