A 5.00 L flask with mass of 463.873 g is filled with Ar gas to 3 atm pressure at 292 k. (19 celsius + 273) what is the mass of flask and gas?
Use the gas law equation and solve for n (moles):
PV=nRT
Where
P=3 atm
V=5.00L
R= 0.0821 liter·atm/mol·K
T=292K
and
n=???
Solve for n:
n=PV/RT
n*39.95g/mol=mass of gas
***You can perform the rest.
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To find the total mass of the flask and gas, we need to consider the mass of the flask and the mass of the gas separately, and then add them together.
First, let's calculate the mass of the flask. The mass of the flask can be obtained by subtracting the mass of the gas from the total mass of the flask and gas.
Given:
Mass of flask = 463.873 g
Next, let's find the volume of the flask. The volume of the flask is given as 5.00 L.
Now let's determine the density of argon gas. The density of a gas can be calculated using the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in K)
Rearranging the equation to solve for n (moles):
n = PV / RT
Given:
P = 3 atm
V = 5.00 L
T = 292 K
We need to convert the temperature from Celsius to Kelvin by adding 273 to it, so T = 292 K.
Now, let's calculate the number of moles of argon gas:
n = (3 atm * 5.00 L) / (0.0821 L.atm/mol.K * 292 K)
Now that we have the number of moles of argon gas, we can calculate the mass of the gas using the molar mass of argon.
The molar mass of argon (Ar) is approximately 39.95 g/mol.
Given:
Molar mass of argon (Ar) = 39.95 g/mol
Mass of gas = number of moles * molar mass
Now, let's calculate the mass of the gas:
Mass of gas = n * molar mass
Finally, we can find the total mass of the flask and gas:
Total mass = Mass of flask + Mass of gas
Hence, calculate the mass of flask and gas using the given information by following the steps outlined above.