A 3.00- flask is filled with gaseous ammonia, . The gas pressure measured at 28.0 is 1.25 . Assuming ideal gas behavior, how many grams of ammonia are in the flask?
To determine the number of grams of ammonia in the flask, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = amount of substance (in moles)
R = ideal gas constant
T = temperature
First, we need to convert the given temperature from Celsius to Kelvin by adding 273.15 to it.
28.0 °C + 273.15 = 301.15 K
Next, we convert the pressure from atm to Pa (Pascal) by multiplying it by 101,325 (1 atm = 101,325 Pa).
1.25 atm * 101,325 Pa/atm = 126,656.25 Pa
Next, we rearrange the ideal gas law equation to solve for n:
n = PV / RT
Substituting the values into the equation:
n = (126,656.25 Pa) * (3.00 L) / [(0.0821 L · atm / K · mol) * (301.15 K)]
Simplifying the equation:
n = (379,968.75 L · Pa) / (24.925 L · atm / K · mol)
n = 15229.86 mol
Finally, we need to convert the amount of substance from moles to grams using the molar mass of ammonia (NH3), which is approximately 17.03 g/mol.
grams = (15229.86 mol) * (17.03 g/mol)
grams = 259,542.46 g
Therefore, there are approximately 259,542.46 grams of ammonia in the 3.00 L flask.