Analysis Calculate the moles of CO2 using PV = nRT. Calculate the molar mass of

Question

Analysis Calculate the moles of CO2 using PV = nRT. Calculate the molar mass of CO2. Which is more dense, CO2(g) of air? What is your qualitative proof? What is your qualitative proof? What s making the small pieces of CO2 "sing and dance"? What would happen to the final result if the CO2(s) sample was too large (more than enough) to fill the flask? What would happen to the final result if the CO2(s) sample was too small (not enough) to fill the flask? What would happen to the final result if you measure the room temperature (which is higher) instead of CO2 temperature? In step (1), the 'empty' flask actually contains air. If the density of air was given to be 0.00115g/mL, recalculate the molar mass of CO2. You need to calculate the mass of air. Compare the molar mass from analysis2 with Q6. Which one is more accurate? What causes them to be different? Summary: Report the unit used in your latest calculation. For example, if degree C is measured but K is used in the calculation report in K. REMINDER: Are you hand writing all these in ink? Mass ___________ Temperature ____________ Volume ____________ Pressure _________ R ____________ Molar mass of CO2 __________ 19 _________ (from analysis) Molar mass of CO2_43.5 __________ (from Q6) Theoretical molar mass of C0O2 _________ 44 ______ Abstract: No more than 100 words stating why the lab was done, what was done, the major result(s), and conclusion(s). Reflection Statement: One thing I might to differently next time is ..... because ......

Explanation / Answer

Answer:

1) Carbon dioxide has one carbon atom and two oxygen atoms, and a molecular weight of 44 grams per mole. The oxygen in the air is actually O2, or molecular oxygen, with a molecular weight of 32. Hence, carbon dioxide has a higher density, or is heavier than oxygen.

Note : as per chegg guidelines solve first question

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