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1. A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm³, respectively. Calculate the original pressure of the gas in (i) bar, (ii) atm. A vessel of volume 22 1 dm3 contains 2.0 mol H and 1.0 mol N at 273 15 K initially AII

1. A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm³, respectively. Calculate the original pressure of the gas in (i) bar, (ii) atm. A vessel of volume 22 1 dm3 contains 2.0 mol H and 1.0 mol N at 273 15 K initially AII

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.127QP: A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000...
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1. A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm³, respectively. Calculate the original pressure of the gas in (i) bar, (ii) atm. 2. A vessel of volume 22.4 dm³ contains 2.0 mol H2 and 1.0 mol N, at 273.15 K initially. All the H2 reacted with sufficient N, to form NH3. Calculate the partial pressures and the total pressure of the final mixture. 3. Assume that air consists of N2 molecules with a collision diameter of 395 pm. Calculate (i) the mean speed of the molecules, (ii) the mean free path, (ii) the collision frequency in air at 1.0 atm and 25 °C. 0.50 m® Pa mol2. Its volume is 4. A certain gas obeys the van der Waals equation with a found to be 5.00 × 104m³ mol1 at 273 K and 3.0 MPa. From this information, calculate the van der Waals constant b. What is the compression factor for this gas at the prevailing temperature and pressure?
Transcribed Image Text:1. A perfect gas undergoes isothermal compression, which reduces its volume by 2.20 dm³. The final pressure and volume of the gas are 5.04 bar and 4.65 dm³, respectively. Calculate the original pressure of the gas in (i) bar, (ii) atm. 2. A vessel of volume 22.4 dm³ contains 2.0 mol H2 and 1.0 mol N, at 273.15 K initially. All the H2 reacted with sufficient N, to form NH3. Calculate the partial pressures and the total pressure of the final mixture. 3. Assume that air consists of N2 molecules with a collision diameter of 395 pm. Calculate (i) the mean speed of the molecules, (ii) the mean free path, (ii) the collision frequency in air at 1.0 atm and 25 °C. 0.50 m® Pa mol2. Its volume is 4. A certain gas obeys the van der Waals equation with a found to be 5.00 × 104m³ mol1 at 273 K and 3.0 MPa. From this information, calculate the van der Waals constant b. What is the compression factor for this gas at the prevailing temperature and pressure?
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