They tell us how many grams of the carbon dioxide we have and how many grams of the water we have, they tells us that right over there. I could try to, even with the x's and y's, but that's not the point of this video. And what I just drew here, this is a chemical reaction Presence of molecular oxygen and it's going to combust and after it's combusted, I'm going to end up with someĬarbon dioxide and some water. It only contains carbon and hydrogen, so it's going to have To make sure we understand what's going on. What is the empiricalįormula of the compound? So pause this video and see if you can work through that. Density: Calculate the average density of carbon dioxide from your data.That a sample of a compound containing only carbon and hydrogen atoms is completely combusted, producing 5.65 grams of carbon dioxide and 3.47 grams of H2O or water. Use this value to calculate the percent error in your average experimental molar mass for carbon dioxide. Accepted molar mass of CO2 and percent error: Calculate the accepted molar mass of carbon dioxide from the molar masses of carbon and oxygen. Calculate the average molar mass from your three trials.Ħ. Molar mass of CO: Calculate the experimental molar mass of carbon dioxide for each trial using the ideal gas law. Mass of CO2: Calculate the mass of carbon dioxide in the flask for each trial from part 3 of the procedure and part 3 of the calculations. Mass of empty flask: Calculate the true mass of the empty flask from the value in part 2 of the procedure and the value in part 2 of the calculations. Mass of air in flask: mar = (density of air) (flask volume) = (1.13 g/L) x V (from part 5. Tand P: Convert the pressure in inches of mercury (in Hg) into atm (29.92 in Hg = 1 atm). Usc 0.998 g/mL for the density of the water to find the volume (V). Add the last bits of water with a dropper to fill the flask. ![]() Alternatively you can weigh the water in the flask by first taring the flask on the balance, then carefully adding water to it. Make sure you estimate the volutne (V) to the nearest 0.1 mL. Determine the volume of the flask by filling it with water (finish filling the flask using a dropper) and then measuring the water with a graduated cylinder. Repeat the dry ice sublimation two more times (using the same Erlenmeyer flask and piece of foil) so that you have a total of three sets of values for m2 5. When the solid has completely sublimed, squeeze the cap tightly on the flask, dry the condensed moisture of the bottom and weigh again and record as m. Obtain a small piece (0.3-0.5 g) of dry ice (solid CO2) and put it in the flask. Weigh the flask and the cap (and the air inside the flask) and record as m. Do not fit the cap tightly on the flask at this time. Get a piece of aluminum foil and make a cap for the flask by laying the foil over the mouth of the flask and folding it down over the sides. Procedure Note: Use the balance that measures milligrams, 0.001 g, for all masses today. Molar mass is found by dividing the weight of the gas by the number of moles of gas, n. The constant Ris 0.0821 L'atm/mol K, so P must be in atm, Vin liters and 7 in Kelvin. ![]() ![]() The number of moles of gas, n, is found by using the ideal gas law, n - PV/RT. Introduction In this experiment you will find the molar mass of carbon dioxide, CO2, by determining the pressure, volume, temperature and mass of the gas phase. Molar Mass Objective To determine the molar mass of CO2 by gravimetric analysis of gases.
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