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Thermodynamics, Statistical Thermodynamics, & Kinetics
- A glass tumbler containing 243 cm3 of air at 1.00 102 kPa (the barometric pressure) and 20C is turned upside down and immersed in a body of water to a depth of 25.5 m. The air in the glass is compressed by the weight of water above it. Calculate the volume of air in the glass, assuming the temperature and barometric pressure have not changed.arrow_forwardAt the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forwardIn the discussion on the composition of air, mention is made of the fact that water vapor may have a concentration as high as 40,000 ppm. Calculate the partial pressure exerted by water vapor at this concentration. Assume that this represents a situation with 100% humidity. What temperature would be needed to achieve this value? (See Appendix G.)arrow_forward
- A 2.0 L soda bottle is pressurized with 4.5 atm of CO2 at 298 K. If the temperature is increased to 317 K, what is the pressure of the CO2?arrow_forwardThe density of air at 20C and 1.00 atm is 1.205 g/L. If this air were compressed at the same temperature to equal the pressure at 50.0 m below sea level, what would be its density? Assume the barometric pressure is constant at 1.00 atm. The density of seawater is 1.025 g/cm3.arrow_forwardA breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at a barometric pressure of 101.4 kPa, if PHe = 82.5 kPa and PCO2 = 0.4 kPa?arrow_forward
- A sample of 4.5 moles of an unknown gas occupies a volume of 1.6L at 23.2atm, what is the ideal temperature in oC for this sample of gas? A student attempted to solve the above problem in the pic below, but made an error in the process. Identify the error or errors, solve the problem correctly, and provide the correct answer.arrow_forwardA sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.24 L1.24 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 30.0 atm,30.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V= Larrow_forward9.41 mol of argon gas is admitted to an evacuated 9,472.23 cm3 container at 46.51oC. The gas then undergoes an isochoric heating to a temperature of 242.1oC. What is the final pressure?arrow_forward
- Gay-Lussac’s Law The temperature of a sample of gas in a steel tank at 30.0 kPa is increasedfrom –100.0 ̊ to 1.00 x 103 ̊C to 25.0 ̊. What is the final pressure inside the tank?arrow_forwardA manometer consists of a U-shaped tube containing a liquid. One side is connected to the apparatus and the other is open to the atmosphere. e pressure p inside the apparatus is given p = pex + ρgh, where pex is the external pressure, ρ is the mass density of the liquid in the tube, g = 9.806 m s−2 is the acceleration of free fall, and h is the difference in heights of the liquid in the two sides of the tube. ( the quantity ρgh is the hydrostatic pressure exerted by a column of liquid.) (i) Suppose the liquid in a manometer is mercury, the external pressure is 760 Torr, and the open side is 10.0 cm higher than the side connected to the apparatus. What is the pressure in the apparatus? the mass density of mercury at 25 °C is 13.55 g cm−3. (ii) In an attempt to determine an accurate value of the gas constant, R, a student heated a container of volume 20.000 dm3 filled with 0.251 32 g of helium gas to 500 °C and measured the pressure as 206.402 cm in a manometer filled with water at 25…arrow_forward
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