What volume a sample of 67.0 grams of nitrogen gas (N2)will occupy at -25degrees C and 3 atm pressure?
Use PV = nRT
T must be in kelvin.
To find the volume of a given sample of nitrogen gas (N2) at a specific temperature and pressure, we can use the ideal gas law equation: PV = nRT.
Given:
Mass of nitrogen gas (N2) = 67.0 grams
Temperature = -25 degrees Celsius (convert to Kelvin)
Pressure = 3 atm
Step 1: Convert the temperature to Kelvin.
To convert from Celsius to Kelvin, simply add 273.15 to the temperature value.
Temperature (Kelvin) = -25 + 273.15 = 248.15 K
Step 2: Convert the mass of nitrogen gas (N2) to moles.
We need to convert the mass of the gas to moles using the molar mass of nitrogen gas, which is 28.0134 grams/mole.
Moles of N2 = Mass of N2 / Molar mass of N2
Moles of N2 = 67.0 g / 28.0134 g/mol ≈ 2.392 mol
Step 3: Plug the values into the ideal gas law equation and solve for volume.
PV = nRT
P = Pressure = 3 atm
V = Volume (to be determined)
n = Moles = 2.392 mol
R = Ideal Gas Constant = 0.0821 L∙atm/(mol∙K)
T = Temperature (Kelvin) = 248.15 K
Rearrange the equation to solve for V:
V = (nRT) / P
Plug in the values:
V = (2.392 mol * 0.0821 L∙atm/(mol∙K) * 248.15 K) / 3 atm
Calculate the volume:
V ≈ 40.8 L
Therefore, a sample of 67.0 grams of nitrogen gas (N2) will occupy approximately 40.8 liters at -25 degrees C and 3 atm pressure.