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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- A 7.00 L tank at 6.54 °C is filled with 17.3 g of sulfur tetrafluoride gas and 17.7 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: х10 sulfur tetrafluoride partial pressure: | atm ? mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atmarrow_forwardA sample of an unknown compound is vaporized at 100.°C . The gas produced has a volume of 1330.mL at a pressure of 1.00atm , and it weighs 4.52g . Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits.arrow_forward1) A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. 2) According to the ideal gas law, a 1.092 mol sample of oxygen gas in a 1.698 L container at 275.0 K should exert a pressure of 14.51 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L2atm/mol2 and b = 3.183×10-2 L/mol.3) According to the ideal gas law, a 9.702 mol sample of nitrogen gas in a 0.8232 L container at 500.8 K should exert a pressure of 484.3 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.arrow_forward
- A 10.12 mol sample of argon gas is maintained in a 0.8094 L container at 304.4 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. atmarrow_forwardAccording to the ideal gas law, a 0.9575 mol sample of methane gas in a 1.064 L container at 273.0 K should exert a pressure of 20.16 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For CH4 gas, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.arrow_forward5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)arrow_forward
- 150. g of an unknown monatomic gas phase element has just been released into a container of volume 90.95 L at a pressure of 1.0114 atm. If the temperature of the room is 25.4°C, what are the molar mass and the identity of the gas? molar mass identity of the gasarrow_forwardA sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 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 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.arrow_forwardThe critical pressure, Pe, and the critical temperature, Te, of gas A are 3.040 × 10° Pa and 473 K, respectively. (i) Calculate the van der Waals constants, a and b, for this gas. (ii) Gas A obeys the van der Waals equation. Calculate the pressure exerted by one mole of gas A if the molar volume occupied by this gas is 2.75 L/mol at 298 K.arrow_forward
- Use the ideal gas equation to calculate the pressure exerted by 1.380 mol of Cl2 in a volume of 5.255 L at a temperature of 249.0 K .arrow_forwardCalculate the amount of nitrogen gas in moles collected at 762.39 torr and 21.2˚ C if the gas has a volume of 15209 mL. The gas was not collected over water.The ideal gas constant, R = 82.1 atm·mL/mol·K.The ideal gas equation is: PV=nRTarrow_forwardAccording to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a 4.194 L2atm/mol² and b 5.105×102 L/mol. Percent difference = |Pideal - Pvan der Waals x 100 Pideal + Pvan der Waals % 2arrow_forward
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