A mixture of methane gas, CH, (), and propane gas, C,H, (), has a pressure of 0.6205 bar when placed in a sealed container. The complete combustion of the mixture to carbon dioxide gas, Co, G), and water vapor, H,O(g), was achieved by adding exactly enough oxygen gas, O,(g), to the container. The pressure of the product mixture in the sealed container is 2.486 bar. Calculate the mole fraction of methane in the initial mixture assuming the temperature and volume remain constant.

A mixture of methane gas, CH, (), and propane gas, C,H, (), has a pressure of 0.6205 bar when placed in a sealed container. The complete combustion of the mixture to carbon dioxide gas, Co, G), and water vapor, H,O(g), was achieved by adding exactly enough oxygen gas, O,(g), to the container. The pressure of the product mixture in the sealed container is 2.486 bar. Calculate the mole fraction of methane in the initial mixture assuming the temperature and volume remain constant.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.32E

See similar textbooks

Similar questions

perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure complete combustion of CH4 to CO2(g) and H2O(g), three times as much oxygen as is necessary is reacted. Assuming air is 21 mole percent O2 and 79 mole percent N2, calculate the flow rate of air necessary to deliver the required amount of oxygen. b. Under the conditions in part a, combustion of methane was not complete as a mixture of CO2(g) and CO(g) was produced. It was determined that 95.0% of the carbon in the exhaust gas was present in CO2. The remainder was present as carbon in CO. Calculate the composition of the exhaust gas in terms of mole fraction of CO, CO2, O2, N2, and H2O. Assume CH4 is completely reacted and N2 is unreacted.
The Berthelot equation of state for one mole of gas is p=RTV-b-aTV2 Where a and b are constants determined experimentally. For NH3g, a = 741.6 atm. L2. K and b = 0.0139 L. Calculate p when V=22.41L and T = 273.15K. How much does the pressure vary from p as predicted by the ideal gas law?
Under what conditions of temperature does a Redlich-Kwong gas behave like an ideal gas? Use the Redlich-Kwong equation of state to justify your answer.
Carbon monoxide poisoning results when carbon monoxide replaces oxygen bound to hemoglobin. The oxygenated form of hemoglobin, HbO2 carries O2 to the lungs. HbO2(aq)+CO(g)HbCO(aq)+O2(g) At 98.6°F (37°C), G° for the reaction is about -14 kJ. What is the ratio of [HbO2] to [HbCO] when the pressure of CO is the same as that of O2?
Use the ideal gas law to demonstrate the cyclic rule of partial derivatives.
When two cotton plugs. one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
Butane gas, C4H10, is sold to campers as bottled fuel. Its density at 25C and 1.00 atm is 2.38 g/L. What volume of butane gas at 25C and 1.00 atm is required to heat one gallon of water (d=1.00g/mL) from 25C to 98C ? The reaction for the combustion of butane (H f =125.6kJ/mol) is C4H10(g)+132 O2(g)4CO2(g)+5H2O(g)
Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?
Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KClO3(s) completely decomposes into O2(g) and KCl(s). However, MnO2(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KClO3(s) and 100. mg of MnO2(s) were mixed in a testube and heated over a bunsen burner. The resulting O2(g) product was bubbled in distilled water that is at exactly 25 °C (or 298.15 K) and collected in a 100-mL eudiometer. The experiment was done under a barometric pressure of 755 torr. The vapor pressure of water vapor at 25 °C is 23.8 mmHg. After reacting for several seconds, the heat was removed, and the contents of the test tubes containing the remaining KClO3(s), the MnO2(s) catalyst, and the KCl(s) product was weighed to be 1.285 g. The level of the liquid inside the eudiometer rests 1.36 cm below the water level in the reservoir. The graduation on the eudiometer indicates that…
An ideal gas confined to a container with a massless piston at the top. A massless wire is attacted to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45L. When the external pressure is increased to 2.50 atm, the gas futher compresses from 2.45 to 1.96L In a seperate experiment with the same initial conditions of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96L in one step. If the final temperture was the same for both processes, what is the difference between q for the two step pocess and q for the one process in joules?
a 1.2 mol sample of oxygen is placed in a 20L tank at 100kPa, whta is tthe tank temperature?