Use PV = nRT and solve for n = moles.
Then moles = grams/molar mass. You know moles and molar mass, solve for grams.
Then moles = grams/molar mass. You know moles and molar mass, solve for grams.
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature. Thus, 22.3°C + 273.15 = 295.45 K.
Now, we rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (1.1 atm)(13.3 L) / (0.0821 L·atm/mol·K)(295.45 K)
Simplifying:
n = 18.058 mol
Since the molar mass of nitrogen (N2) is 28.014 g/mol, we can calculate the number of grams of gas present:
Number of grams = number of moles × molar mass
Number of grams = 18.058 mol × 28.014 g/mol
Number of grams ≈ 505.7 g
Therefore, the sample of nitrogen gas present in the container weighs approximately 505.7 grams.