A 3.00- L
flask is filled with gaseous ammonia, NH3
. The gas pressure measured at 20.0 ∘C
is 2.05 atm
. Assuming ideal gas behavior, how many grams of ammonia are in the flask?
To find the number of grams of ammonia in the flask, we can use the ideal gas law equation:
PV = nRT
where:
P = pressure (in atm)
V = volume (in L)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in K)
First, we need to convert the temperature from Celsius to Kelvin:
T = 20.0 + 273.15
T = 293.15 K
Now we can rearrange the ideal gas law equation to solve for the number of moles of ammonia:
n = PV / RT
n = (2.05 atm)(3.00 L) / (0.0821 L·atm/mol·K)(293.15 K)
n = 0.250 moles
To find the mass of ammonia in grams, we can use the molar mass of ammonia (NH3), which is 17.03 g/mol:
mass = number of moles * molar mass
mass = 0.250 moles * 17.03 g/mol
mass = 4.26 grams
Therefore, there are 4.26 grams of ammonia in the flask.