A flexible plastic container contains 0.833 g of helium gas in a volume of 18.3 L. If 0.203 g of helium is removed at constant pressure and temperature, what will be the new volume?
V=.203/.833 * 18.3 Liters
To find the new volume, we need to use the ideal gas law, which states: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
First, we need to find the initial number of moles using the given mass of helium gas. The molar mass of helium (He) is approximately 4.0026 g/mol.
Number of moles = Mass / Molar mass
Number of moles = 0.833 g / 4.0026 g/mol
Number of moles ≈ 0.2081 mol
Now, let's calculate the initial volume using the ideal gas law:
PV = nRT
Initial volume = (nRT) / P
Given:
Pressure (P) = Constant
Number of moles (n) = 0.2081 mol
Ideal Gas constant (R) = 0.0821 L·atm/(mol·K) (remember to use the appropriate units for R)
Temperature (T) = Constant
Now we can solve for the initial volume:
Initial volume = (0.2081 mol * 0.0821 L·atm/(mol·K) * T) / P
Let's denote the initial volume as V₁.
Now, to find the final volume (V₂), we remove a certain amount of helium gas. The remaining mass of helium gas is:
Remaining mass = Initial mass - Removed mass
Remaining mass = 0.833 g - 0.203 g
Remaining mass = 0.630 g
We can repeat the process to find the final number of moles:
Number of moles = Remaining mass / Molar mass
Number of moles = 0.630 g / 4.0026 g/mol
Number of moles ≈ 0.1574 mol
Finally, we can use the ideal gas law to find the final volume:
Final volume = (Number of moles * 0.0821 L·atm/(mol·K) * T) / P
Let's denote the final volume as V₂.
You will need to substitute the appropriate values for pressure and temperature to calculate the final volume.