1. Write a balanced chemical equation that describes the reactions that took place. What volume of oxygen is necessary to burn 0.1 g of lighter fluid? What volume of carbon dioxide is produced?
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.
PLEASE ANSWER THE QUESTION BASE ON THE PROBLEM GIVEN BELOW
QUESTION
1. Write a balanced chemical equation that describes the reactions that took place. What volume of oxygen is necessary to burn 0.1 g of lighter fluid? What volume of carbon dioxide is produced?
PROBLEM
While the rest of the family was finishing up a game of volleyball in the bright afternoon sunshine. Brendon attempted to start a fire in the charcoal grill. He arranged the charcoal briquettes and squirted them with lighter fluid. He waited a few minutes for the fuel to soak into the charcoal and then he lit the pile of charcoal briquettes with a match. Flames from the match quickly begun to ignite the briquettes.
Just as the fire got going. Brendon’s brother knocked the volleyball out of bounds and Brendon ran to get it. By the time he returned the ball and chatted with the family, the fire appeared to have gone out. Brendon grabbed the can of lighter fluid and squeezed it sides to douse the charcoal again. Suddenly, the can of lighter fluid exploded, spewing burning fluid everywhere. Luckily, Brendon dropped the can---not a fraction of a second too soon---and was spared serious injury.
The moral of this story is never to add lighter fluid to charcoal twice. Use the following information to determine exactly why this is true. A typical molecule of lighter fluid might be C7H16. A molecule like this one, consisting of carbon and hydrogen, is called a hydrocarbon. When hydrocarbons are ignited by heat, as from the flame of a match, they combine with oxygen in the air in a combustion reaction.
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