According to the ideal gas law, a 10.12 mol sample of krypton gas in a 0.8350 L container at 495.1 K should exert a pressure of 492.4 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/mol? and b = 3.978×10² L/mol. [Pideal – Pvan der Waals| x 100 Percent difference Pideal+P der Waals van

According to the ideal gas law, a 10.12 mol sample of krypton gas in a 0.8350 L container at 495.1 K should exert a pressure of 492.4 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/mol? and b = 3.978×10² L/mol. [Pideal – Pvan der Waals| x 100 Percent difference Pideal+P der Waals van

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...

See similar textbooks

Similar questions

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.25 atm, and the mole fraction of O2 in air is 0.210.
For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is lowered from 19.0°C⁢ to −17.0°C, and at the same time the pressure is changed. If the initial pressure was 2.2 atm and the volume decreased by 45.0%, what is the final pressure?
A sample of gas contains 0.1500 mol of CH₁ (g) and 0.3000 mol of O₂(g) and occupies a volume of 19.3 L. The following reaction takes place: CH4 (9) +202(g) → CO₂(g) + 2H₂O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume = L
According to the ideal gas law, a 10.24 mol sample of xenon gas in a 0.8381 L container at 499.4 K should exert a pressure of 500.7 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a 4.194 L²atm/mol² and b = 5.105×102 L/mol. = Percent difference | Pideal – Pvan der Waals | × 100 Pideal+Pvan der Waals % 2
A sample of an ideal gas at 1.00 atm and a volume of 1.67 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 70.0 atm, what was the volume of the sample? Assume that the temperature was held constant. L V = 41.9
An ideal gas is contained in a cylinder with a volume of 5.1*10^2 mL at a temperature of 30.°C and a pressure of 710. torr. The gas is then compressed to a volume of 27 mL, and the temperature is raised to 820.°C. What is the new pressure of the gas? Pressure = torr
According to the ideal gas law, a 1.024 mol sample of xenon gas in a 1.047 L container at 272.4 K should exert a pressure of 21.86 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b = 5.105×10-2 L/mol.
7.) A glass bulb contains an unknown gas. The gas is either CO2, SO2, C2H6, or CH3F. Here is some data that was collected for this gas sample. Use the data to identify the unknown gas. Mass of glass bulb with the unknown gas: 14.402 g Volume of glass bulb: 670. mL Mass empty bulb 12.232 g Pressure 1751. torr Temperature 21.oC
1) A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. 2) According to the ideal gas law, a 1.092 mol sample of oxygen gas in a 1.698 L container at 275.0 K should exert a pressure of 14.51 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L2atm/mol2 and b = 3.183×10-2 L/mol.3) According to the ideal gas law, a 9.702 mol sample of nitrogen gas in a 0.8232 L container at 500.8 K should exert a pressure of 484.3 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.
According to the ideal gas law, a 0.9575 mol sample of methane gas in a 1.064 L container at 273.0 K should exert a pressure of 20.16 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For CH4 gas, a = 2.253 L2atm/mol2 and b = 4.278×10-2 L/mol.
5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)
Gaseous ammonia is synthesized from nitrogen and hydrogen by the reaction N2(g) + 3H2(g)→ 2NH3(g) Assume you take 355 L of H2 gas at 25.0 °C and 542 mm Hg and combine it with excess N2 gas. a )What is the theoretical yield of NH3 gas? b) If this amount of NH3 gas occupies a 125-L tank at 25.0 °C, what is its pressure?