Problems 1 find the location of a nearby barometer go

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PROBLEMS1.Find the location of a nearby barometer. Go there and measure thepressure of the atmosphere. Make a careful drawing of the pointer andscale on the barometer showing the pressure as you read it.
PROBLEMS105If no barometer is available, you can go to almost any weather websiteand find the current atmospheric pressure for the nearest weather station.Now, to run yourself through all these terms and units, make a tablewith two rows and eight columns. In the first row label each column withthe name of a unit of pressure. Using the appropriate units, put the valueof the pressure that you measured into each column of the second row.Why is the number you measured different from the value of the“standard atmosphere”?2.Suppose you have a piston with an area of 100 cm2sitting on a volumeof 10 L of nitrogen gas atT= 20C. If the gas is heated and warmedtoT= 30C, by how much does the volume change? Give your answeraccurate to±1%.3.Suppose you have a pyrex flask that has a volume of 350 mL at 0C.What will be its volume after being heated to 100C?4.State the argument by which the ideal gas law is determined. Derivethe ideal gas law from Boyle’s Law and Gay-Lussac’s Law.5.State the ideal gas law, identify the variables in the law, and use it tofind the pressure of 1 mole of gas contained in a volume of 11.2 L at 0C.6.A 45-liter container at room temperature is known to have in it atotal ofN= 15×1023diatomic molecules of oxygen gas.a.What is the number densitynof the molecules of this gas? Giveyour answer in units of cm3.b.What is the number of moles,nM, of this gas?c.What is the pressure of this gas?7.An experimenter measures pressure of gas as its volume is changedand gets the following data:Pressure (Pa)Volume (m3)10001.515001.020000.752500
1064.GAS LAWSa.Do these data obey Boyle’s law? Explain how you know.b.What value of volume would you expect to measure for the missingentry in the above table?8.Suppose the above data were taken at a temperature of 27C and thenlater the gas was cooled to73C. At what volume would the cooled gashave a pressure of 1000 Pa?9.Consider the following table of measurements of pressure vs. volumefor O2(MO2= 32 u) in a closed container at 300 K.Pressure (kPa)Volume (cm3)90.924.8973.630.7359.537.93a.Is it reasonable to conclude that the gas obeys Boyle’s law? Howdid you come to this conclusion? Discuss clearly.b.How many molecules are contained in this volume? How do youknow?c.If the oxygen molecules are replaced by an equal number of heliumgas molecules (MHe= 4 u) at the same temperature, what wouldbe the gas pressure when the volumeV= 30.73 cm3? (Hint: Seethe above table.)10.Boyle’smeasurement of the air pressure outside his apparatus(Fig.4.6) was 29216inches of mercury (Hg). [The density of Hg isρHg=13.6 g cm3.]292/16"FIGURE 4.6Barometer for Problem10.

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Term
Fall
Professor
NG, Yee Fai
Tags
Atom, Modern Introductory Physics