A 3.00-
L
flask is filled with gaseous ammonia,
N
H
3
. The gas pressure measured at 28.0
∘
C
is 2.05
atm
. Assuming ideal gas behavior, how many grams of ammonia are in the flask?
Use PV = nRT and solve for n = number of mols.
Then grams = mols x molar mass = ?
Post your work if you get stuck. Remember to use kelvin for T.
To calculate the number of grams of ammonia in the flask, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atmospheres)
V = volume of the gas (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 28.0 + 273.15
T(K) = 301.15 K
Next, let's rearrange the ideal gas law equation to solve for moles:
n = (PV) / (RT)
Now, we can substitute the given values into the equation:
n = (2.05 atm) * (3.00 L) / (0.0821 L·atm/(mol·K)) * (301.15 K)
Calculating this equation will give us the number of moles of ammonia in the flask. Finally, to calculate the mass, we need to use the molar mass of ammonia, which is 17.03 g/mol. Multiply the molar mass by the number of moles to get the mass:
Mass = n * Molar mass
Mass = (n) * (17.03 g/mol)
Perform these calculations to find the mass of ammonia in grams.