sectional view through a submarine. Atmospheric pressure is 101 kPa‚ and sea water density is 1020 kg/m3. Determine the depth of submergence y. 1 BPH – Tut # 2 Question 4 In the dry adiabatic model of the atmosphere‚ in addition to the ideal gas equation‚ air is also assumed to obey the equation p/ρn = constant where n = 1.4. If the conditions at sea level are standard (101.3 kPa‚ 15°C)‚ determine the pressure and temperature at an altitude of 4000 m above sea level. Solutions. Q
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ANSWERS 391 ANSWERS Chapter 9 9.1 9.2 1.8 (a) From the given graph for a stress of 150 × 106 N m-2 the strain is 0.002 (b) Approximate yield strength of the material is 3 × 108 N m-2 9.3 (a) Material A (b) Strength of a material is determined by the amount of stress required to cause fracture: material A is stronger than material B. 9.4 9.5 9.6 9.7 9.8 9.9 9.10 9.11 9.12 9.13 9.14 9.15 9.16 (a) False (b) True 1.5 × 10-4 m (steel); 1.3 × 10-4 m (brass) Deflection
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(isothennal w-s atm- 1 at 20 °C; find out (!lin SI unit. [2) (d) In the gas-phase reaction A+ 2B ~ 3C + 2 D‚ it was found that when 2.00 mol A‚ 1.00 mol B‚ and 3.00 molD were mixed and allowed to come to equilibrium at 25°C‚ the resulting mixture contained 0.79 mol Cat a total pressure of 1.00 bar. Calculate (i) Kx‚ (ii) Kpand (iii) ~Gr • The 0 symbols carry usual meaning. Assume the gases are ideal. [2+1+1] [P.T.O.] L - ·- ---------- - - - -__ _ _ _ _ _! Q2. (a) Standard
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change in temperature and pressure of ethanol using a Vernier temperature probe. By using the ideal gas equation‚ and plugging the slope value from the graph into the Clausius-Claypernon equation‚ enthalpy of vaporization was determined to be 10kJ/mol. The percent error was determined to be 76.0%. Introduction: The purpose of this lab is to investigate vapor pressures and the partial pressure of gas produced from liquids at different temperatures. These pressures vary at different temperatures
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Name of the Student:………………… Date:………….. What is the volume of 1 mole of hydrogen gas? One mole of any gas occupies the same volume when measured under the same conditions of temperature and pressure. In this experiment you will calculate the volume of 1 mole of hydrogen at room temperature and pressure. Intended lesson outcomes By the end of this practical you should be able to: • further develop skills in manipulating apparatus and accurate measurement; • use the mole concept; • calculate
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First the total volume of gas that is to be stored needs to be calculated. From the mass balance it is known that 30.92 kmol of methane can be expected every hour. This correlates to 742.0 kmol/day. The ideal gas law will be used‚ with a compressibility factor‚ Z‚ to account for departure for un-idealality. An operating temperature of 50 will be assumed‚ as this is the highest feasible ambient temperature that can be expected. Also assume that the pump or compressor used to transport the methane
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are ideal‚ however‚ this does not exist in reality. a. State the conditions under which gases deviate from ideal behaviour and explain why the deviations occur. [4] __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ b. Sketch a graph of PV versus P showing the curves for an ideal gas
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ABSTRACT This experiment was carried out to determine the relationship between the pressure and the temperature of saturated steam in equilibrium. Besides that this experiment was also done to demonstrate the vapor pressure curve. The marcet Boiler was used for this experiment. When the pressure increases‚ the temperature also increases. Therefore‚ the relationship of pressure and temperature is directly proportional. The derived formulae and the data were used to calculate the slope. The dT/dP
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Molar Volume of a Gas – 10/27/08 Alic Albright‚ Josh Coleman‚ Dan Boden‚ Zach Babin Purpose: The pupose of this lab was to make an experimental determination of a molar volume through reaction of the substance shown: Mg(s) + 2HCl(aq) > MgCl(aq) + H(g) Introduction: In this lab‚ a magnesium ribbon and HCl are combined in a gas measuring tube. When they are combined they form magnesium chloride and Hydrogen gas. The molar ratio between Mg reacted and
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of the volume occupied by a gas is empty space. This accounts for the lower density of gases compared to liquids and solids‚ and the fact that gases are easily compressible.<br><br>b) The particles of a gas are in constant motion‚ moving rapidly in straight lines in all directions‚ and thus passes kinetic energy. The kinetic energy of particles overcomes
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