The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V andtemperature I for gases better than the Ideal Gas Law does:72(V-nb)= nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas.The parameters a and b must be determined for each gas from experimental data.Use the van der Waals equation to answer the questions in the table below.What are the units of a?What are the units of b?For argon the numerical value of a is 1.337 and the numericalvalue of b is 0.0320.Use the van der Waals equation to calculate the pressure of asample of argon at -110.0 °C with a molar volume of 2.98 L/molRound your answer to the correct number of significant digits.atmUse the Ideal Gas Law to calculate the pressure of the samesample under the same conditions. Round your answer to thecorrect number of significant digits.atmx10§

Step 1: Step 2: Step 3: Step 4:

Answered: The van der Waals equation of state was…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 7.13 L cylinder contains 1.82 mol of gas A and 3.77 mol of gas B, at a temperature of 31.8 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior. PA= PB = What is the total pressure? PTotal = kPa kPa kPa
Calculating partial pressure in a gas mixture esc A 7.00 L tank at 29. °C is filled with 6.44 g of chlorine pentafluoride gas and 13.6 g of boron trifluoride 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. Round each of your answers to 3 significant digits. chlorine pentafluoride boron trifluoride R Explanation 2 mole fraction: W partial pressure: Total pressure in tank: 2 mole fraction: partial pressure: Check #3 8.0 E 54 https://azinsight.adsrvr.org/track/clk?imp=fbec12b0-713d-4127-929d-a59782e61fbb&ag=r735012&sfe=1788cd47&sig=PCK7icABpePPZol9wVL E9gKn0Pi6FOTr7R3rMUmfWw.&crid=2zvfx50b&cf=5773664&fq=0&t=2&tds-www.chegg.com&rca $ a F4 0 R atm 0 atm atm % 5 X FS T Ś < 6 s F6 Y & 7 F7 U 00 8 DIL FB 1 ( 9 DD ) O 0/5 Danasia V O F10 . P Fad d da delet
A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the storage unit rises to 76 °C, causing the gas to decompose and doubling the number of moles in the cylinder. Note: R = 0.08206 Latm/molK Determine the moles of gas in the cylinder before any decomposition occurs. Determine the pressure in the cylinder after the decomposition in atmospheres.
Calcium carbonate, CaCO3(s), decomposes upon heating to give CaO(s) and CO2(g). A sample of CaCO3 is decomposed, and the carbon dioxide is collected in a sealed 250 mL flask. After the decomposition is complete, the gas has a pressure of 1.6 atm at a temperature of 33°C. How many moles of CO2 gas were generated? (Ideal gas equation: PV = nRT.)
13
Arrange the following gases in the order of increasing deviation from ideal gas behavior. Assume the identical condition of temperature and pressure. CO2 Cl2, Kr van der Waals Constants of Some Comimon Gases atm L mol Gas mol Не Ne 0.034 0.211 0.0237 0.0171 0.0322 0.0398 0.0266 0.0266 Ar 1.34 Kr 2.32 Xe H2 N2 4.19 0.244 1.39 0.0391 O2 Cl2 CO, 1.36 0.0318 0.0562 0.0427 0.0428 6.49 3.59 2.25 CH, CC, NH, 20.4 4.17 5.46 0.138 0.0371 0.0305 HO Select one: O a. Cl2 < CO2 < Kr O b. CO2 < C2< Kr O c Kr < Cl2 < CO2 O d. CO2 < Kr - Cl2 O e. Kr < CO2 Cl2 O f. Cl2 < Kr < CO2
One of the factors that influences the behavior of a gas sample is pressure. Pressure can be expressed using different units, and it is important to be able to convert between them. Convert a pressure of 0.413 atm to mm Hg. Convert a pressure of 2.9 kPa to units of mm Hg.
A 4.17 g4.17 g sample of NH3NH3 gas and a 4.17 g4.17 g sample of HClHCl gas are mixed in a 2.00 L2.00 L flask at 25 ∘C. What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH4ClNH4Cl produced by the reaction.
A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen difluoride 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. sulfur hexafluoride dinitrogen difluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm atm atm x10 olo 18 Ar
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If pressure is expressed in atmospheres and volume is expressed in liters, PAV has units of L atm (liters x atmospheres). Remember that 1 atm 101,325 Pa, and that 1 L = 1 dm³. Use this information to determine the number of joules corresponding to 2L atm. eTextbook and Media Savo for Lotor
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