What is the density of sulfur dioxide gas at 25 degrees celsius and 754 mm Hg?
To find the density of sulfur dioxide gas at a specific temperature and pressure, we need to use the ideal gas law and the molar mass of sulfur dioxide.
The ideal gas law equation is:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature
In this case, we are given the temperature (25 degrees Celsius or 298 Kelvin) and the pressure (754 mm Hg or 1 atm = 760 mm Hg). However, we don't have the volume or the number of moles.
Assuming we have 1 mole of sulfur dioxide gas, we can rearrange the ideal gas law equation to solve for the volume:
V = nRT/P
Substituting the given values:
V = (1 mol) * (0.0821 L·atm/(mol·K)) * (298 K) / (1 atm)
V = 24.3848 L
Now that we have the volume, we can calculate the density using the formula:
Density = mass / volume
To find the mass, we need to know the molar mass of sulfur dioxide (SO2). The molar mass of sulfur (S) is 32.06 g/mol and the molar mass of oxygen (O) is 16.00 g/mol.
So, the molar mass of sulfur dioxide is:
Molar mass (SO2) = (32.06 g/mol) + 2 * (16.00 g/mol)
= 64.06 g/mol
Assuming 1 mole of sulfur dioxide gas, the mass will be equal to the molar mass (64.06 g).
Now we can calculate the density:
Density = mass / volume
Density = (64.06 g) / (24.3848 L)
Density ≈ 2.62 g/L
Therefore, the approximate density of sulfur dioxide gas at 25 degrees Celsius and 754 mm Hg is 2.62 g/L.