Elemental analysis is performed on an organic liquid with a fishy odor. Vaporization of 260.0 mg of the compound in a 110 mL bulb at 100°C gives a pressure of 410.0 torr. What is the molar mass of this compound?

whats the formula for this and do I need to convert anything?

Use PV = nRT and solve for n. You must convert 410 torr to atm and 100 C to kelvin.

Then n = grams/molar mass.
You know n and grams. Solve for molar mass.

To determine the molar mass of the compound, we can use the ideal gas law equation:

PV = nRT

where:
P = pressure (410.0 torr)
V = volume (110 mL or 0.110 L)
n = number of moles of the compound
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (100°C = 273.15 + 100 = 373.15 K)

First, let's rearrange the equation to solve for n (number of moles):

n = (PV) / (RT)

Now, substitute the given values into the equation:

n = (410.0 torr * 0.110 L) / (0.0821 L·atm/mol·K * 373.15 K)

Before we proceed further, we need to convert the pressure from torr to atm and the volume from mL to L, as the ideal gas constant has units in atm, L, and Kelvin.

To convert torr to atm, divide by 760:
410.0 torr / 760 = 0.539 atm

To convert mL to L, divide by 1000:
0.110 mL / 1000 = 0.110 L

Substituting these values back into the equation:

n = (0.539 atm * 0.110 L) / (0.0821 L·atm/mol·K * 373.15 K)

Now, we can calculate the number of moles (n) using a calculator:

n ≈ 0.00307 mol

Since molar mass is defined as the mass of one mole of a substance, we need to find the mass of the compound. Given that 260.0 mg of the compound was vaporized, we can convert this mass to grams by dividing by 1000:

260.0 mg / 1000 = 0.260 g

Now, we can determine the molar mass of the compound by dividing the mass by the number of moles:

Molar mass = mass / moles
Molar mass = 0.260 g / 0.00307 mol

Calculating this, we find:

Molar mass ≈ 84.7 g/mol

Therefore, the molar mass of the compound is approximately 84.7 g/mol.