Some N2 gas is mixed with some O̟2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured,and found to be 2.55 atm.keycarbonhydrogennitrogensulfuroxygenchlorineCalculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as anideal gas.gasmole fractionpartial pressurex10atmN₂02☑atm

Answered: Image /qna-images/answer/28fe26bf-be13-4aeb-bc89-244da16348bc.jpg

Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 2.55 atm. key carbon hydrogen nitrogen oxygen sulfur chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an deal gas. gas mole fraction partial pressure ☐ x10 N2 ☐ atm 02 0 ☐ atm 5

Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 2.55 atm. key carbon hydrogen nitrogen oxygen sulfur chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an deal gas. gas mole fraction partial pressure ☐ x10 N2 ☐ atm 02 0 ☐ atm 5

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

ChapterC: Mathematics For General Chemistry

Section: Chapter Questions

Problem 2P

See similar textbooks

Similar questions

Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do this, calculate a 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). On a graph show the apparent molar mass versus the 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?
How would the use of a volatile liquid affect the measurement of a gas using open-ended manometers vs. closed-end manometers?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Consider these four gas samples, all at the same temperature. The larger boxes have twice the volume of the smaller boxes. Rank the gas samples with respect to: (a) pressure, (b) density, (c) average kinetic energy, and (d) average molecular speed. (Green spheres are He; violet spheres are Ne.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
A 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?