Calculate what mass of argon gas is required to full a 20.4-L container to a pressure of 1.09 atm at 25C
36.3g Ar
Use PV = nRT
To calculate the mass of argon gas required to fill a 20.4-L container to a pressure of 1.09 atm at 25 degrees Celsius, you can use the ideal gas law equation: PV = nRT.
First, let's convert the given pressure and volume values to standard units:
Pressure: 1.09 atm
Volume: 20.4 L
Next, we need to convert the temperature to Kelvin. Celsius and Kelvin scales are related by the equation T(K) = T(°C) + 273.15. So, 25°C equals 25 + 273.15 = 298.15 K.
Now we have all the necessary values to calculate the number of moles of argon gas (n). The ideal gas law equation can be rearranged to solve for n:
n = PV / RT
Where:
P is the pressure in atm,
V is the volume in liters,
R is the ideal gas constant (0.0821 L.atm/mol.K), and
T is the temperature in Kelvin.
Substituting the values into the equation:
n = (1.09 atm) * (20.4 L) / (0.0821 L.atm/mol.K * 298.15 K)
Now we can calculate the number of moles:
n = 0.894475 mol
Finally, we need to convert moles of argon gas to mass using the molar mass of argon. The molar mass of argon (Ar) is approximately 39.95 g/mol.
Mass = n * molar mass = 0.894 mol * 39.95 g/mol
Calculating the mass:
Mass = 35.73 g
Therefore, the mass of argon gas required to fill the 20.4-L container to a pressure of 1.09 atm at 25°C is approximately 35.73 grams.