What volume in liters is occupied by 8.22 g of SO2 gas confined at a pressure of 1200.8 torr at 75.0*c?
Use PV = nRT where n = grams/molar mass.
To find the volume occupied by the gas, we can use the Ideal Gas Law equation, which states:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, let's convert the given values to suitable units:
Pressure: 1200.8 torr can be converted to atm by dividing by 760 torr/atm.
1200.8 torr / 760 torr/atm = 1.58 atm
Temperature: 75.0°C can be converted to Kelvin by adding 273.15.
75.0°C + 273.15 = 348.15 K
Now, we can rearrange the Ideal Gas Law equation to solve for volume:
V = (nRT) / P
To determine the number of moles of SO2 gas, we need the molar mass of SO2. The molar mass of S = 32.06 g/mol, and O = 16.00 g/mol. Therefore,
Molar Mass of SO2 = (1 x Molar Mass of S) + (2 x Molar Mass of O)
Molar Mass of SO2 = (1 x 32.06 g/mol) + (2 x 16.00 g/mol)
Molar Mass of SO2 = 64.06 g/mol
Now, we can calculate the number of moles (n) using the given mass:
n = mass / molar mass
n = 8.22 g / 64.06 g/mol
n = 0.1281 mol
Substituting the values into the equation:
V = (nRT) / P
V = (0.1281 mol x 0.0821 L.atm/mol.K x 348.15 K) / 1.58 atm
V = 3.44 liters
Therefore, the volume occupied by 8.22 g of SO2 gas under the given conditions is 3.44 liters.
To calculate the volume occupied by the SO2 gas, we can use the Ideal Gas Law equation, which is given by:
PV = nRT
Where:
P = pressure in atmospheres (torr can be converted to atm by dividing by 760)
V = volume in liters
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (°C can be converted to Kelvin by adding 273.15)
First, let's convert the pressure from torr to atm:
1200.8 torr ÷ 760 = 1.579 atm
Now, let's convert the temperature from Celsius to Kelvin:
75.0°C + 273.15 = 348.15 K
Next, we need to calculate the number of moles of SO2 gas. To do this, we can use the formula:
n = mass / molar mass
The molar mass of SO2 is sulfur (32.06 g/mol) + oxygen (2 * 16.00 g/mol) = 64.06 g/mol.
n = 8.22 g / 64.06 g/mol = 0.128 mol
Now, we can substitute these values into the Ideal Gas Law equation:
(1.579 atm) * V = (0.128 mol) * (0.0821 L·atm/mol·K) * (348.15 K)
Simplifying:
V = (0.128 mol * 0.0821 L·atm/mol·K * 348.15 K) / 1.579 atm
V ≈ 3.52 liters
Therefore, 8.22 g of SO2 gas confined at a pressure of 1200.8 torr and temperature of 75.0°C occupies approximately 3.52 liters of volume.