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In analyzing and solving gas law problems, it is helpful to tabulate the information given in the problems and then to convert the values to units that are consistent with those for R (0.08206 L-atm/mol-K). In this case the given values are Remember: Absolute temperature must always be used when the ideal-gas equation is solved.
At 20 ºC, glycerol (d = 1.261 g/mL) is used in an open-end manometer instead of mercury (d = 13.55 g/mL). Calculate the gas pressure (in atm) if the level of the arm to the gas is 62.5 cm higher than the level to the atmosphere. The atmospheric pressure is 0.942 atm.
Problem #1: A mixture of 40.0 g of oxygen and 40.0 g of helium has a total pressure of 0.900 atm. What is the partial pressure of each gas? Solution: 1) Calculate moles of each gas: He: 40.0 g / 4.0026 g/mol = 9.9935 mol O 2: 40.0 g / 31.9988 g/mol = 1.25005 mol. 2) Calculate mole fraction: He: 9.9935 mol / 11.24355 mol = 0.88882
Define the property of pressure; Define and convert among the units of pressure measurements; Describe the operation of common tools for measuring gas pressure; Calculate pressure from manometer data
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We can use the ideal gas equation to calculate the volume of 1 mole of an ideal gas at 0°C and 1 atmosphere pressure. First, we have to get the units right. 0°C is 273 K. T = 273 K
Use ideal gas law P(100.0L) = 5.0(8.31)(300.0) P = 125 kPa *10. A 50.0 L sealed cylinder contains 100.0 moles of helium gas. Its pressure at 273 K is 44.80 atm. What is the change in pressure when the gas is heated to 500.0 K? If moles are the same, you can compare pressure and temperature together by combining the laws 𝑷𝒊𝑽𝒊
