CHM 2045 Lecture Notes - Circulatory System, Reynolds Number, Blood Vessel

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byzantiumjackal692

24 Feb 2014

School

University of Florida

Department

Chemistry

Course

CHM 2045

Professor

chu

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Specific gravity of a material is defined as the ratio of its density to the density of water at 4 degrees c (also known as relatve density) i. The pressure pint at the level of the oil-water interface in the left arm depends on density and height of the oil i. c. For a given pressure, the heiht of the mercury column does not depend on the cross sectional area of the vertical tube b. c. For a given pressure, the height of the column of mercury depends on the value of g at the location of the barometer and on the density of mercury, which varies with temperature. Measures the gauge pressure pg of a gas. Consist of a u-tube containing liquid, which one end of the tube connected to a vessel whose gauge pressure we wish to measure and the other end open to the atmosphere.

Related Questions

Show all the steps:

1) what will be the hydrogen pressure?

2) what will be the mass of Magnesium?

3) what will be the moles of hydrogen?

4) what will be percent by mass Mg?

can someone help me with this showing all steps? Thanks in advance.

Percent Magnesium in a Mixture Background In th is experiment you will determine the percent magnesium in a mixture containing only magne- sium and zine by reacting the sample with hydrochloric acid and measuring the volume of hydroger gas evolved. The reactions are: From the volume of hydrogen collected and its temperature and pressure, gen generated can be calculated. Using the stoichiometric relationships shown in the reactions above and knowing the total mass of zinc and magnesium, equations can be set up to solve for the individu al masses of the metals. the total moles of hydro- Determining the pressure of the hydrogen is a litle bit tricky. The hydrogen is collected over acid solution in a long calibrated tube called a gas measuring tube or eudiometer whi a beaker of water. The hydrogen pressure is not the barometric pressure. The total pressure in the eudiometer a ch is inverted in t the level of the liquid in the beaker is equal to the barometric pressure. This is the gas pressure plus the pressure due to the acid column above the liquid level in the beaker. To deter- mine the gas pressure barometric pressure. The column abo ure the pressure due to the acid column must be found and subtracted from the pressure of the acid column can be found by measuring the height of the ve the level of liquid in the beaker. Since we measure pressure as the height of a mercury column, the acid column height must be converted to mm Hg. The height of a liquid column sup- ported by a given pressure is inversely proportional to the density of the liquid. The density of the acid in the eudiometer is 1.05 e/mL and the density of mercury is 13.6 2/mL. Since the gas above the acid solution is hydrogen plus be subtracted from the gas pressure to get the pressure of the hydrogen alone. This is the pressure you will use in your calculations. Aqueous vapor pressures can be found in the table in Appendix C in your lab manual, or in the CRC Handbook which is available from the stockroom. water vapor and not pure hydrogen, the aqueous vapor pressure must pensi mercurs- 13.69/mL Volu me gas53. a melnic pressure 30 psi heiant of acal column 35.3 cm mass ââ corlonel metals= o.or68q

I need the ones that I did checked, and c, f, l, and m done please.

Molar Volume of Oxygen Experiment

Before you can start this experiment, you must: Solve problems I, II, and III Pass an 8 question on-screen computer quiz In problems I, II, and III:

Calorimeter constant is 0.00 j/Â°C Specific Heat of water or aqueous solutions is 4.18 j/g Â°C I. 89.6542 g of metal were heated to 101.1 Â°C and poured into a calorimeter containing 49.60 g of water at 27.35 Â°C. After stirring, the temperature of the water rose rapidly to 34.75 Â°C before slowly starting to fall. Calculate:

a) The Specific Heat of the metal _____________

b) The Atomic Weight _____________

Calculated using the rule of Dulong and Petit II.

To a calorimeter containing 41.90 g of water at 25.00 Â°C, 7.6039 g of a salt was added with stirring. As the salt dissolved, the temperature rapidly changed to 27.95 Â°C before slowly returning to room temperature.

Calculate:c) The Heat of Solution ______________ Given that the Heat of Formation of the solid salt is.... -228.24 Kj/mol and the Molecular Mass of the solid salt is.......... 67.22 g/mol

Calculate: d) The Heat of Formation of the Solution ______________ Kj/mol III. Given the reaction... AAA + BBB ---> CCC You add to a calorimeter 10.0 mL of 4.19 M AAA, 9.0 mL of water, and 12.0 mL of 5.14 M BBB. All of the above solutions were initially at 29.95 Â°C. After mixing, the temperature changed to 32.80 Â°C. Assume the density of all solutions is 1.000 g/mL and all solutions have the same specific heat as pure water.

Calculate: e) The Heat of Reaction in Kj/mol ______________

CHM 2045 Lecture Notes - Circulatory System, Reynolds Number, Blood Vessel

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