1.Suppose you have a container filled with air at 212 oF. The volume of the container 1.00 L, the pressure of air is 1.00 atm. The molecular composition of air is 79% N2 and 21% O2 for simplification. Calculate the mass of air and moles of O2 in the container.moles of O2=.006 and moles of N2=.025 moles 2.A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container(total mass of air=.892) , according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container? I need help with finding the new total pressure for question 2.
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
1.Suppose you have a container filled with air at 212 oF. The volume of the container 1.00 L, the pressure of air is 1.00 atm. The molecular composition of air is 79% N2 and 21% O2 for simplification. Calculate the mass of air and moles of O2 in the container.moles of O2=.006 and moles of N2=.025 moles
2.A small portion of gaseous gasoline (boiling point of gasoline: ~185 oF, it becomes gas at 212 oF) was then injected to mix with air in the container(total mass of air=.892) , according to air/fuel ratio (14.7:1 by mass). Consider 90% mass of gasoline is isooctane and the rest is ethanol (C2H6O), how much are isooctane and ethanol in moles added, respectively? With the amount of gasoline injected, what is new total pressure of the container?
I need help with finding the new total pressure for question 2.
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