To solve this problem, we can use the ideal gas law:
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, let's convert the volume to liters and the temperature to Kelvin:
Volume = 1900 mL = 1.9 L
Temperature = 120°C = 120 + 273.15 = 393.15 K
Now, we can rearrange the ideal gas law to solve for the number of moles:
n = (PV) / RT
Substituting the given values:
n = (1.00 atm * 1.9 L) / (0.0821 L atm / mol K * 393.15 K)
n ≈ 0.0476 moles
Next, we'll calculate the molar mass (M) using the formula:
M = mass / moles
Substituting the given mass:
M = 2.00 g / 0.0476 moles
M ≈ 42.017 g/mol
Rounding to three significant digits, the molar mass of the compound is approximately 42.0 g/mol.
