A 355.0 ml container holds 0.146 g nitrogen gas and an unknown amount of argon at 35 degrees and a total pressure of 626 mmHg, Calculate the amount (mol) of argon in the container.
which is the container
To calculate the amount (mol) of argon in the container, we need to use the ideal gas law equation:
PV = nRT
Where:
P is the pressure in atm
V is the volume in liters
n is the amount of gas in moles
R is the gas constant (0.0821 L.atm/mol.K)
T is the temperature in Kelvin
First, let's convert the given volume from milliliters to liters:
355.0 ml = 355.0/1000 = 0.355 L
Next, we need to convert the given pressure from millimeters of mercury (mmHg) to atm:
626 mmHg = 626/760 = 0.8237 atm
Now, we can rearrange the ideal gas law equation to solve for n (the amount of gas in moles):
n = PV / RT
Let's substitute the given values:
n = (0.8237 atm * 0.355 L) / (0.0821 L.atm/mol.K * 35 + 273.15 K)
= 0.2922 / (2.8735 + 273.15)
= 0.2922 / 276.0235
Finally, we can calculate the amount of argon in moles:
n = 0.00105800659 mol
Therefore, there is approximately 0.0011 mol of argon in the container.