MolecularWeight

MolecularWeight - of the flask to hold .155 liters. Using...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Molecular Weight of a Volatile Liquid 1/16/08 Introduction In this lab, we were able to find the formula weight of any substance using a container with a known volume. We used a substance in liquid form, then heated it enough to vaporize the substance to fill a container. This determined the volume (it is equal to the volume of the container), and weighed it to find the mass. With this data, the calculations to find the formula weight can be completed. Chemical Responsibility When dealing with our unknowns, we should assume they are toxic and flammable. In addition, they are colored with iodine, so they should not come into contact with the skin. Results My unknown was a purple liquid, unknown #664. My first experiment yielded . 471 grams of the vapor. My second experiment yielded .521 grams. I found the volume
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: of the flask to hold .155 liters. Using the given barometric pressure (765 mmHg), I was able to calculate the molecular weight for each experiment. I calculated them to be 92.25 g/mol and 101.77 g/mol, an average of 97.01 g/mol. Conclusion We were able to find these calculations because of how easily measurable the physical properties of this lab were. The pressure of the vapor was just the atmospheric pressure as the flask was left open to the atmosphere. The temperature is the temperature of the boiling water. The mass was the difference in mass of the empty flask and the vapor filled flask. Care must be taken to be accurate as possible, as this could create a large margin of error....
View Full Document

This note was uploaded on 08/15/2008 for the course CHM U215 taught by Professor Lui during the Spring '08 term at Northeastern.

Ask a homework question - tutors are online