Question 1
(a) Use the ideal gas equation to calculate the pressure (in atm) of 2.40 mol of krypton (Kr) at 455 K in a 4.50 L vessel. (b) In a 16.3 L vessel, the pressure of 2.40 mol of Kr at 455 K is 5.50 atm when calculated using the ideal gas equation and 5.40 atm when calculated using the van der waals equation of state (Note: a=5.121 and b = 0.0106). Why is the percent difference in the pressure calculated using the different equations greater when the gas is in the 4.50 L vessel compared to the 16.3 L vessel? (select from the following):
____ The molecular volume is a smaller part of the total volume of the 4.50 L vessel
____ The attractive forces between molecules become less of a factor at the higher pressure in the 4.50 L vessel.
____ The attractive forces between molecules become a greater factor at the higher pressure in the 4.50 L vessel
____ The molecular volume is a larger part of the total volume of the 4.50 L vessel
Question 1 (a) Use the ideal gas equation to calculate the pressure (in atm) of 2.40 mol of krypton (Kr) at 455 K in a 4.50 L vessel. (b) In a 16.3 L vessel, the pressure of 2.40 mol of Kr at 455 K...
Use the van der Waals equation of state to calculate the pressure of 2.40 mol of H2S at 499K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. In a 16.30 L vessel, the pressure of 2.40 mol of H2S at 499 K is 6.03 atm when calculated using the ideal gas equation and 5.97 atm when calculated using the...
Use the van der Waals equation of state to calculate the pressure of 2.10 mol of Kr at 471 K in a 3.70L vessel. Van der Waals constants can be found in this table. Number P- 2.004 atm Use the ideal gas equation to calculate the pressure under the same conditions. Number P= 21.947 atm In a 15.5 L vessel, the pressure of 2.10 mol of Kr at 471 K is 5.24 atm when calculated using the ideal gas equation...
- A 1.31 mol sample of Kr gas is confined in a 32.4 liter container at 28.0 °C. If the temperature of the gas sample is raised to 43.1 °C holding the volume constant, the average molecular speed will a) not enough information to answer the question b) decrease c)remain the same d) increase -Which of the following statements is true for real gases? Choose all that apply. Attractive forces between molecules cause a decrease in pressure compared to the...
Use the van der Waals equation of state to calculate the pressure of 2.30 mol of CH, at 455 K in a 5.50 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. atm Under these conditions, would you expect CH, or CCI, to deviate more from ideal behavior? Why? OCCI, because it occupies a larger volume and it has greater...
According to the ideal gas law, a 0.9054 mol sample of krypton gas in a 1.023 L container at 274.0 K should exert a pressure of 19.90 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. % According to the ideal gas law, a 9.344 mol sample of oxygen gas in a 0.8267 L container at 500.1...
1: according to the ideal gas law, a 1.016 mol sample of Krypton gas is in a 1.875 liter container at 273.8 Kelvin should exert a pressure of 12.17 atmospheres by what percent does the pressure calculated using the boundary waals equation differ from the ideal pressure? for Kr gas, a=2.318 L^2 ATM/mol^2 and b=3.978x10^-2 2: the average molecular speed in a sample of O3 gas at a certain temperature is 399 m/s. the average molecular speed in a sample...
Use the van der Waals equation of state to calculate the pressure of 3.70 mol of CCI4 at 499K in a 3.70 L vessel. Van der Waals constants can be found in the van der Waals constants table. Use the ideal gas equation to calculate the pressure under the same conditions. In a 15.00 L vessel, the pressure of 3.70 mol of CCI4 at 499 K is 10.1 atm when calculated using the ideal gas equation and 9.2 atm when calculated using...
According to the ideal gas law, a 10.74 mol sample of krypton gas in a 0.8444 L container at 498.7 K should exert a pressure of 520.5 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. ____%
According to the ideal gas law, a 0.9935 mol sample of krypton gas in a 1.258 L container at 265.4 K should exert a pressure of 17.20 atm. By what percent does the pressure calculated using the van der Waals' equation differ from the ideal pressure? For Kr gas, a - 2.318 L'atm/mol- and b= 3.978*10-2 L/mol. Hint: % difference = 100*(P ideal - Pvan der Waals) /P ideal
The ideal pressure of 1.00 mol CH3Cl gas in a 4.50 L flask at 100.0 K is 1.82 atm. What is its real pressure? For CH3Cl: a = 7.570 atm∙L2 /mol2 b = 0.06483 L/mol a. 1.27 atm b. 1.45 atm c. 1.48 atm d. 1.51 atm e. 1.58 atm