5. Compare the values obtained for the pressure of 3.00 mol CO₂ at 298.15 K held in a 8.25-dm³ bulb using the ideal gas and van der Waals (real gas) equations. 6. A particular mass of N, occupies a volume of 1.00 L at-50 °C and 800 bar. Determine the volume occupied by the same mass of N₂ at 100 °C and 200 bar using the compressibility factor for N₂. At-50 °C and 800 bar it is 1.95; at 100 °C and 200 bar it is 1.10. Compare this value to that obtained from the ideal gas law.

5. Compare the values obtained for the pressure of 3.00 mol CO₂ at 298.15 K held in a 8.25-dm³ bulb using the ideal gas and van der Waals (real gas) equations. 6. A particular mass of N, occupies a volume of 1.00 L at-50 °C and 800 bar. Determine the volume occupied by the same mass of N₂ at 100 °C and 200 bar using the compressibility factor for N₂. At-50 °C and 800 bar it is 1.95; at 100 °C and 200 bar it is 1.10. Compare this value to that obtained from the ideal gas law.

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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Question

5. Compare the values obtained for the pressure of 3.00 mol CO₂ at 298.15 K held in a 8.25-dm³ bulb using
the ideal gas and van der Waals (real gas) equations.
2
6. A particular mass of N₂ occupies a volume of 1.00 L at-50 °C and 800 bar. Determine the volume occupied
by the same mass of N₂ at 100 °C and 200 bar using the compressibility factor for N₂. At -50 °C and 800 bar
it is 1.95; at 100 °C and 200 bar it is 1.10. Compare this value to that obtained from the ideal gas law.

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