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 0.090 kPa. key carbon O hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 2 significant digits. You may assume each gas behaves as an ideal gas.

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 0.090 kPa. key carbon O hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 2 significant digits. You may assume each gas behaves as an ideal gas.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 97E: Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation: HN3O(g)N2(g)+H2(g)...

See similar textbooks

Similar questions

Referring to exercises 1.6 and 1.7, does it matter if the pressure difference is caused by an ideal gas or a non-ideal gas? Explain your answer.
Explain why the plot of PV for CO2 differs from that of an ideal gas.
Hydrogen azide, HN3, decomposes on heating by the following unbalanced equation: HN3O(g)N2(g)+H2(g) If 3.0 atm of pure HN3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
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?
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.