A 200-mg sample of a purified compound of unknown molar mass is dissolved in benzene and dilut ed with that solvent to a volume of 25.0 cm^3. The resulting solution is found to have an osmotic pressure of 0.010 5 atm at 300 K. What is the molar mass of the unknown compound?

Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7$\%$ nitrogen and 80.3$\%$ fluorine by mass, and determine the formal charge of the atoms in this compound.

What is the main difference between qualitative and quantitative observations?

The following procedure is a simple through somwhat crude way to measure the molar mass of a gas. A liquid of mass 0.0184 g is introduced into a syringe like the one shown here by injection through the rubber tip using a hypodermic needle. The syringe is then transferred to a temperature bath heated to 45 °C, and the liquid vaporizes. The final volume of the vapor (measured by the outward movement of the plunger) is 5.58 mL, and the atmospheric pressure is 760 mmHg. Given that the compounds's empiricial formula is $\mathrm{CH_2}$, determine the molar mass of the compound.

A 0.15-g sample of a purified protein is dissolved in water to give 2.0 mL of solution. The osmotic pressure is found to be 18.6 torr at $25^{\circ} \mathrm{C}.$ Calculate the protein’s molar mass.