Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 1, Problem 1.52E
Under what conditions of volume does a van der Waals gas behave like an ideal gas? Use the van der Waals equation of state to justify your answer.
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Chapter 1 Solutions
Physical Chemistry
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- Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?arrow_forwardAt high temperatures, one of the van der Waals constants can be ignored. Which one? Justify your choice and write a high temperature version of the van der Waals equation of state.arrow_forwardWhat properties of a nonideal gas do the Vander Waals constants represent?arrow_forward
- Under what conditions would the van der Waals constant b be negative? Do you think there are any gases for which this occurs?arrow_forwardWhy is nitrogen a good choice for the study of ideal gas behavior around room temperature?arrow_forwardGiven that 1.00 mol of neon and 1.00 mol of hydrogen chloride gas are in separate containers at the same temperature and pressure, calculate each of the following ratios. (a) volume Ne/volume HCI (b) density Ne/density HCI (c) average translational energy Ne/average translational energy HCI (d) number of Ne atoms/number of HCl moleculesarrow_forward
- Calculate the Boyle temperatures for carbon dioxide, oxygen, and nitrogen using the van der Waals constants in Table 1.6. How close do they come to the experimental values from Table 1.5?arrow_forwardOxygen Consumption If 5.00 L of hydrogen gas,measured at a temperature of 20.0°C and a pressure of80.1 kPa, is burned in excess oxygen to form water, whatmass of oxygen will be consumed? Assume temperatureand pressure remain constant.arrow_forwardStarting with the definition of rate of effusion and Graham’s finding relating rate and molar mass, show how to derive the Graham’s law equation, relating the relative rates of effusion for two gases to their molecular masses.arrow_forward
- 2. The species identified with each curve in the Maxwell-Boltzmann plot below are: (Assume all gases are at the same temperature.) A = Xe, B = O2, C = Ne, and D = He A = Xe, B = He. C = Ne, and D = O2 A = He, B = Ne, C = O2, and D = Xe A = He, B = O2, C = Ne, and D = Xe Molecular speed (m/s)arrow_forwardA 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?arrow_forwardScottish physicist W. J. M. Rankine proposed an absolute temperature scale based on the Fahrenheit degree, now called degree Rankine abbreviated R and used by some engineering fields. If a degree Rankine is 5/9 of a degree Kelvin, what is the value of the ideal gas law constant in L. atm/mol. R?arrow_forward
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