Please correct answer and don't use hand rating GasesUnderstanding Boyle's Law35LorA cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 81.6 kPa.The piston is now pushed down, compressing the gas, until the gas has a final volume of 1.90 L. Calculate the final pressure of the gas. Round your answer to 3significant digits.kPapistoncylindergas

The problem involves using Boyle's Law, which states that for a given mass of an ideal gas at…

Answered: Gases Understanding Boyle's Law 35 Lor…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 20QAP

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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.
Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressure
Explain why the plot of PV for CO2 differs from that of an ideal gas.
Describe the factors responsible for the deviation of the behavior of real gases from that of an ideal gas.
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.
The hydrocarbon octane (C8H18) bums to give CO2 and water vapor: 2 C8H18(g) + 25 O2(g) 16 CO2(g) + 18 H2O(g) If a 0.048-g sample of octane burns completely in O2, what will be the pressure of water vapor in a 4.75-L flask at 30.0 C? If the O2 gas needed for complete combustion was contained in a 4.75-L flask at 22 C, what would its pressure be?
Butyl mercaptan, C4H9SH, has a very bad odor and is among the compounds added to natural gas to help detect a leak of otherwise odorless natural gas. In an experiment, you burn 95.0 mg of C4H9SH and collect the product gases (SO2, CO2, and H2O) in a 5.25-L flask at 25 C. What is the total gas pressure in the flask, and what is the partial pressure of each of the product gases?
A mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?
5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?
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.
What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 C and 74-4 torr?
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.)

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