A 3.00- flask is filled with gaseous ammonia, . The gas pressure measured at 28.0 is 2.35 . 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 is the pressure of the gas in atm
V is the volume of the gas in liters
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature of the gas in Kelvin
First, we need to convert the given temperature in Celsius to Kelvin by adding 273.15:
28.0 °C + 273.15 = 301.15 K
Next, we rearrange the equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (2.35 atm) * (3.00 L) / (0.0821 L·atm/(mol·K) * 301.15 K)
Calculating:
n ≈ 0.287 mol
Finally, we can convert moles to grams using the molar mass of ammonia (NH3), which is 17.03 g/mol:
grams of ammonia = n * molar mass of ammonia
grams of ammonia ≈ 0.287 mol * 17.03 g/mol
grams of ammonia ≈ 4.89 g
Therefore, there are approximately 4.89 grams of ammonia in the flask.