Chem 142 Lap Postlab Report #5

Chem 142 Lap Postlab Report #5 - EXP 5 MOAR MASS OF A LOW...

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DATA AND CALCULATIONS A. Unknown # 1 Run 1 Run 2 Run 3 Mass of flask + cap + air 44.470 44.470 49.9 Mass of flask + cap + vapor 44.470 44.460 49.88 B. Barometric pressure 762.40 mm Hg = 1 atm Sample temperature 100.00 C = 373.15 K Water (room) temperature 21.600 C = 294.75 K Mass of flask + cap + water 173.96 g Density of water at RT 1 g/mL Volume of Flask, L 0.12 1. Calculate the volume of the flask.(2 pt) density = mass/volume --> d=mass/V V= mass/d V= (173.958g - 49.899g) x 1 L (.99777g/ml) 1000mL = .124336 L EXP 5: MOAR MASS OF A LOW BOILING LIQUID Grading WebAssign prelab: 5 pts This template: 30 pts Lab Notebook Duplicate: 5 pts By signing below, you certify that you have not falsified data and that you have not plagiarized any part of this lab report. Failure to sign this declaration will cost you 5 points. Signature: Purpose and Method Things to think about: What is the goal of this experiment? Explain how it is accomplished. What is the general method (not step by step detailed procedure) that you will be using to achieve this goal? How will you process the data that you record in lab? (What calculations will you use and how do you obtain all of the values to plug into those equations?) (5 points) The goal of this experiment is to determine the molar mass and identity of a liquid that boils at a low temperature. The lab involves heating a liquid until it changes to the gaseous state, at which point we can measure the pressure, volume, and temperature of the gas. These measurements, along with the mass of the gas can be combined in the ideal gas law (PV=nRT) to calculate the molar mass of the sample. n=mass/MM;
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This note was uploaded on 04/06/2008 for the course CHEM 142 taught by Professor Zoller,williamh during the Winter '07 term at University of Washington.

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Chem 142 Lap Postlab Report #5 - EXP 5 MOAR MASS OF A LOW...

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