What is the difference between mass of a cubic meter of gas at sea level and mass of a cubic meter of gas in Denver. Assume a isothermal atmosphere with T=295.
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What is the difference between mass of a cubic meter of gas at sea level and mass of a cubic meter of gas in Denver. Assume a isothermal atmosphere with T=295.
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- Determine at what altitude in meters the air pressure is twice less than on the sea level using the barometic equation that is pressure as a function of height. Given that the temperature is 288.15 K. P=P0e -Mgh/RT, where Po is the pressure at sea level, M is the molar mass of air (in kg/mol), T is standard temperature, R is universal gas constant (8.314 N.m/mol K).The basic barometer can be used to measure the height of a building. If the barometric readings at the top and at the bottom of a building are 675 and 695 mmHg, respectively, determine the height of the building. Take the densities of air and mercury to be 1.18 kg/m3 and 13,600 kg/m3, respectively.A submarine dives down to a depth 80 metres beneath the surface of the ocean. Calculate the pressure in atmospheres at that depth, assuming the density of water is 1029 kg/m3, and the air pressure at the surface is 105.2 kPa. Give your answer with two digits of precision. Note: 1 standard atmosphere is 101325 Pa. Your Answer: Answer
- The city of Denver is 1 mile above sea level. What is the difference in air pressure, in kPa, between Denver and Jacksonville, which is basically at sea level?The oxygen consumption at rest for a 70-kg person is 14.5 liter/h and that 2% of this requirement is provided by the diffusion of oxygen through the skin. Assuming that the skin surface area of the person is 1.7m2 , calculate the diffusion rate for oxygen through the skin in liter/h-cm2.Atmospheric pressure on Earth at its surface is 101 KPa (101 kilopascals or 101,000 N/m2). Which of these statements is true? If we pump out the gas in a closed container leaving only 1 billionth of the original gas there will still be more than 1010 (10 billion) atoms per cm3 in the container. If we pump out the gas in a closed container leaving only 1 billionth of the original gas there will be fewer than 100 atoms per m3 in the container. When we reduce the pressure in the container while keeping the temperature constant, the number of atoms per m3 must stay constant. At 1 atmosphere, the number of atoms/m3 in air at room temperature is about 109, one billion atoms.
- Question 4 : A spherical snowball is melting in such a way that its radius is decreasing at rate of 0.3 cm/min. At what rate is the volume of the snowball decreasing when the radius is 11 cm. (Note the answer is a positive number).Make a plot of pressure vs altitude for a hydrostatic, isothermal atmosphere on Earth, assuming a surface pressure of 1 atm.The surface air on the planet mars is about 0.007atm if you were standing on mars ,the air pressure would be equivalent to a pressure observed at approximately what altitude on earth atmosphere?
- If sea level is 101350pa ,calculate the standard pressure at an altitude of 5000m using (a) the exact formula (b) an isothermal assumption at a standard sea level temperature of 15°C. Is the isothermal approximately adequate?Consider the air above a football field. The field has an area of 5.4x10^3 m^2. Consider the air in the region extending from the ground to 1 m above the surface of the field. Calculate the volume of air in m^3.The density of the atmosphere varies drastically with height, but you can use an average density from sea floor to the space in order to calculate its height. If we approximate this average density to be = 1 Kg/m³, what would be height of the atmosphere? HINT: Since the atmosphere is a fluid (in gas form), you can use the hydrostatic pressure formula (P pgh), just solve for h and use P = 1 atm. BTW, this is how the edge of space is defined, if you make it pass the height of the atmosphere you have reached space :)