0.361g of an unknown liquid occupied a volume of 250.0 ml at 758mm Hg pressure and 100 degrees Celsius. what is the molar mass?

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To find the molar mass of the unknown liquid, we can use the ideal gas law equation:

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 values to the appropriate units:
- Pressure: 758 mm Hg (millimeters of mercury). We need to convert it to atm by dividing it by 760 mm Hg (1 atm = 760 mm Hg).
- Volume: 250.0 ml (milliliters). We need to convert it to liters by dividing it by 1000 ml/l.
- Temperature: 100 degrees Celsius. We need to convert it to Kelvin by adding 273.15 to it.

Converting the values:
Pressure: 758 mm Hg ÷ 760 mm Hg/atm = 0.996 atm
Volume: 250.0 ml ÷ 1000 ml/l = 0.250 L
Temperature: 100 degrees Celsius + 273.15 = 373.15 K

Substituting the values into the ideal gas law equation:

0.996 atm * 0.250 L = n * 0.0821 L·atm/(mol·K) * 373.15 K

Now, let's solve for n (number of moles):

n = (0.996 atm * 0.250 L) / (0.0821 L·atm/(mol·K) * 373.15 K)

n = 0.0592 moles

To find the molar mass, we divide the mass of the substance (0.361g) by the number of moles.

Molar mass = mass / moles
Molar mass = 0.361g / 0.0592 mol

Molar mass ≈ 6.11 g/mol

Therefore, the molar mass of the unknown liquid is approximately 6.11 g/mol.