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 11.0 °C to 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 2.8 atm and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. 0 atm ■ x10 X

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 11.0 °C to 22.0 °C, and at the same time the pressure is changed. If the initial pressure was 2.8 atm and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. 0 atm ■ x10 X

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 38PS: A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The...

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You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
If equal masses of O2 and N2 are placed in separate containers of equal volume at the same temperature, which of the following statements is true? If false, explain why it is false. (a) The pressure in the flask containing N2 is greater than that in the flask containing O2. (b) There are more molecules in the flask containing O2 than in the flask containing N2.
You have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?
A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.
Answer the following questions: (a) If XX behaved as an ideal gas, what would its graph of Z vs. P look like? (b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified? (c) What is the effect of the volume of gas molecules on Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (d) What is the effect of intermolecular attractions on the value of Z? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram. (e) In general, under what temperature conditions would you expect Z to have the largest deviations from the Z for an ideal gas?