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A sample of an unknown compound is vaporized at 120 C . The gas produced has a volume of 1900. mL at a pressure of 1.00 atm , and it weighs 2.00 g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits.

Respuesta :

icetornato
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.

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