A fixed amount of a gas occupies a volume of 4L and exerts a pressure of 410 kPa on the walls of its container. What would be the pressure exerted by the gas if it is completely transferred into a new container having a volume of 9 liters (assuming the temperature and quantity of gas remains constant)?

A fixed amount of a gas occupies a volume of 4L and exerts a pressure of 410 kPa on the walls of its container. What would be the pressure exerted by the gas if it is completely transferred into a new container having a volume of 9 liters (assuming the temperature and quantity of gas remains constant)?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 89QAP

See similar textbooks

Similar questions

What is the van der Waals constant a for Ne in units of bar.cm6/mol2
Photosynthesis by land plants leads to the fixation each year of about 1 kg of carbon on the average for each square meter of an actively growing forest. The atmosphere contains 0.0390% CO₂ by volume. What volume in (m³)of air (25°C, 1 bar) is needed to provide this 1 kg of carbon?
Write all pertinent computations to justify your final answer What is the molecular weight of gas X if it effuses 1.25 times as rapidly asN2?
The ideal gas law also represents the behaviour of mixtures of gases at low pressures. The molar volume of the mixture is the volume divided by the amount of mixture. The partial pressure of gas in a mixture is defined as yiP for an ideal gas mixture, where yi is its mole fraction and P is the total pressure. Ten grams of N2 is mixed with 5 grams of O2 and held at 25oC at 0.750 bar. a. What are the mole fractions of N2 and O2? b. What are the partial pressures of N2 and O2? c. What is the volume of the total mixture?
A container filled with an unknown quantity of the gaseous mixture at 310 K is in hydrostatic equilibrium. At 5 m above the bottom, the pressure is 0.980 bar. At the bottom, the pressure is 1.001 bar. What is the molecular weight of the gaseous mixture?
Which three (3) substances in the table below of van der Waals constants would you expectto deviate most from ideal-gas behavior at low temperature and high pressure? Which three(3) other substances would deviate least? Explain completely with solutions.
At 200atm pressure and 273.15K, PV=17.7dm³atm for 1mol of a gas A and PV=5.6dm³atm for 1mol of gas B. In which gas is the intermolecular force stronger? Explain your answer.
How much carbon dioxide gas (mole percent) is dissolved in a bottle of sparkling water if the manufacturer used a pressure of 2.56 atm in the bottling process at 25°C? HCO2inwater=1630atm and PsatH2O=3.166kPa at 25°C. Assume xH2O=1.
A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.24 L1.24 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 30.0 atm,30.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V= L
Why must the diffusion of gases into or within liquids be presented in terms of partial pressures rather than concentrations?
What is the value of the universal gas constant in J/mol•K (in 3 desimal places, no need to put the unit)
In a system for separating gases, a tank containing a mixtureof hydrogen and carbon dioxide is connected to a much largertank where the pressure is kept very low. The two tanks areseparated by a porous membrane through which the moleculesmust effuse. If the initial partial pressure of each gas is5.00 atm, what will be the mole fraction of hydrogen in thetank after the partial pressure of carbon dioxide has declinedto 4.50 atm?(a) 52.1% (b) 37.2% (c) 32.1% (d) 4.68% (e) 27.4%