A student produced a volatile liquid experiment with the following results:

Mass of flask, boiling water, foil cap, and unkown after cooling, g: 83.350
Mass of flask, boiling stone, and foil cap, g: 82.657
Water bath temperature: 95*C
Barometric pressure: 30.09 in. HG
Volume of flask: 270 mL
Accepted molar mass of unkown, g mol-1: 86.2

What is the density of the vaporized unkown?

What is the molar mass of the vaporized unkown?

Thank you!

To find the density of the vaporized unknown, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

First, let's calculate the number of moles of the vaporized unknown. We can use the ideal gas law equation to determine the number of moles of the vaporized unknown.

Step 1: Calculate the pressure in atm
The given pressure is 30.09 in. Hg. We need to convert it to atm by dividing it by the conversion factor constant, which is 29.92 in. Hg per atm.
Pressure = 30.09 in. Hg / 29.92 in. Hg/atm = 1.00134 atm

Step 2: Convert the temperature to Kelvin
The given temperature is in degrees Celsius. To convert it to Kelvin, we need to add 273.15.
Temperature = 95°C + 273.15 = 368.15 K

Step 3: Convert the volume to liters
The given volume is 270 mL. We need to convert it to liters by dividing it by 1000.
Volume = 270 mL / 1000 = 0.27 L

Now, let's calculate the number of moles (n) using the ideal gas law equation:
PV = nRT
n = PV / RT
n = (1.00134 atm) * (0.27 L) / [(0.08206 L atm/mol K) * (368.15 K)]

Now that you have determined the number of moles, you can proceed to find the density using the given mass of the volatile liquid experiment.

To find the molar mass of the vaporized unknown, you will need to use the formula:

Molar mass (g/mol) = mass (g) / moles

Use the accepted molar mass of the unknown to compare it with the calculated molar mass to assess the accuracy of your experiment.