Final answer:
The calculation involves finding the density of argon gas at -11°C and a pressure of 675 millimeters of mercury (mmHg).
Step-by-step explanation:
To determine the density of argon gas at a temperature of -11°C and a pressure of 675 mmHg, we'll utilize the ideal gas law, given by the equation PV = nRT, where P represents pressure, V is volume, n stands for the number of moles, R denotes the gas constant, and T is temperature. To find the density (density = mass / volume), we'll first compute the number of moles using the ideal gas law equation.
Given conditions:
Temperature (T) = -11°C = 262 K (converted to Kelvin by adding 273.15)
Pressure (P) = 675 mmHg
The molar mass of argon gas is approximately 39.95 grams per mole (g/mol).
Using the ideal gas law formula PV = nRT, we rearrange the equation to solve for the number of moles (n):
n = PV / RT
n = (675 mmHg) × V / (0.0821 L × atm / mol × K × 262 K)
To find the mass (m) of the gas, we rearrange the formula for density (density = mass / volume) to solve for mass:
mass = density × volume
Remember, these calculations assume ideal gas behavior, and real-world conditions might introduce variations due to factors like non-ideal behavior of gases. However, based on the given ideal gas law and calculations, the density of argon gas under the specified conditions can be compute