Air is approximately 80 mol% Nitrogen (M=28kg/kmol) and 20 mol% Oxygen (M = 32kg/kmol). Consider a rigid container of volume 183.4 liters that contains air at P = 2 atm.Throughout this problem, the temperature of the container is maintained fixed and equal to 25 °C. Use the ideal gas law to answer the following questions (R=0.082 m³.atm/kmol.K): Determine the number of moles of N₂ and of O₂ in the container.

Air is approximately 80 mol% Nitrogen (M=28kg/kmol) and 20 mol% Oxygen (M = 32kg/kmol). Consider a rigid container of volume 183.4 liters that contains air at P = 2 atm.Throughout this problem, the temperature of the container is maintained fixed and equal to 25 °C. Use the ideal gas law to answer the following questions (R=0.082 m³.atm/kmol.K): Determine the number of moles of N₂ and of O₂ in the container.

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

Consider a mixture of 2.0 mol He and 1.0 mol Ne in a rigid container at 25˚C and 1.0 bar. Which of these statements are true of this mixture? (There may be more than one!) The helium gas occupies twice as much volume in the container as the neon gas The concentration of helium is twice the concentration of neon in the mixture The two gases have the same average molecular speed Each gas has a partial pressure of 0.5 bar The two gases have the same average kinetic energy
A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 carbon dioxide partial pressure: || atm ? mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: || atm
For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of −196. °C. Suppose the temperature of a sample of nitrogen gas is raised from -23.0 °C to 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.19 kPa and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. kPa x10 × Ś
A gas mixture consists of 0.462 mol hydrogen (H2), 0.705 mol carbon dioxide (CO2), and 2.462 mol nitrogen (N2). If the total pressure of the mixture is 2.82 atm, calculate the partial pressure of each component gas in the mixture.
Determination of the Universal Gas Constant Postlab 1. An evaluation of Rwas performed using the procedures outlined in this exercise, The barometric pressure was 735 torr and the temperature was 21.5 "C. The volume of H2(9) collected was 32.7 mL. The calculated value of Rwas 0.0817 L'atm/mol-K. a. How many grams of Mg metal were used in this determination? 0.0316 70.361 b. If the correction for the vapor pressure of water had not been performed, what would be the calculated value of R? Incorrect c. If the syringe volume had been incorrectly read, resulting in a calculated H, volume of 30.6 mL, what would be the percent error in the calculated value of Rwith respect to the originally calculated value (0.0817 L-atm/mol·K)? 6.4 %
Using the ideal gas law (PV=nRT), calculate how many moles of air are in the lungs of an average person with total lung capacity of 3.2 L? The pressure is 23.9 psi and body temperature is 37∞C. (R= 0.0821 L atm/ mol K) (14.7 psi/1 atm) (K = ∞C + 273).
There are 1.07 X 10-3 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a- |(V-nb) = nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. Ar What are the units of a? What are the units of b? For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. Oat ||atm Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 4.03 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. atm
The combined gas law states that for a fixed amount of gas, the quantity PVIT is constant. This is often expressed by the equation P¡V PV2 T2 where P is the pressure, V is the volume, and T is the temperature, and the subscripts 1 and 2 denote two different conditions. Rearrange the combined gas law to solve for Pj. P = A gas with an initial temperature of 271 K and initial volume of 15.0 L is heated to 317 K and compressed to 10.2 L. The final pressure of the gas is 4.28 atm. What was the initial pressure (P¡) of the gas? P1 = atm
|(V-nb)=DnRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. p+a- v2 The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For argon the numerical value of a is 1.337 and the numerical value of b is 0.0320. atm Use the van der Waals equation to calculate the pressure of a sample of argon at -90.0 °C with a molar volume of 0.192 L/mol . Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm
Consider the following situation: You have a 50 L tank of compressed air at 15 atm and 100 ºC. You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal. The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania). Once the purified air is passed through the getter is it cooled back down to 100 ºC and fills another 50 L storage tank. If air typically contains about 20% oxygen, what could the pressure in the storage tank be? Question 2 options: A) 12 atm B) 15 atm C) 18 atm D) 24 atm