Pressure+and+Temperature.


 * **How temperature affects gases.**

What is a gas? A gas is one of the three forms of matter. Usually, it comes in this order: Solid, Liquid, and then a Gas. For example, the solid form of water is ice, the liquid form of water is water, and the gas form of water is steam. A gas doesn’t have a exact volume or shape. A gas will fill a open space if the space is empty. If it is already another gas in that space, it will mix and move all over the volume of that space. Gas particles, are different from solid and liquid particles because gas particles don’t hang on to each other. This is because their intermolecular force is not strong enough to hold together. These particles are more independent and don’t depend on others. Gases can be pressed together at a large pressure. For example, when you blow up a balloon, volume of air from the atmosphere is being put into the a smaller volume of the balloon causing the balloon to get bigger.

About one gas, Hydrogen. There are many types of gases. For example, hydrogen, nitrogen, oxygen, and noble gases. These are just a few. This gas is invisible, flammable, colorless, tasteless, and odorless. Hydrogen has many uses. Hydrogen’s flame temperature is extremely high and its one of the coldest. At -253 degrees C, hydrogen turns to a liquid. The lightest type of gas is hydrogen, one cubic meter weighs less than 100 grams. Because of fire hazards, hydrogen isn’t used to fill dirigibles and blimps. Now, they substituted it for a combination of helium and hydrogen. Without air, hydrogen is a gas that will not burn or explode. In the air, scientist have found that there are small amounts of hydrogen. Some common uses of hydrogen are in water, table sugar, ammonia, and hydrogen peroxide.



W hat happens when you cool or heat a gas? An example of heating up a gas would be a hot air balloon. When you heat up the balloon, the molecules, spread out, move faster and overall the whole quantity gets less dense, and thus moves up through the cooler air outside. A gas can become a liquid by cooling it to it’s boiling point. Under any kind of pressure that's smaller than 1 atmosphere, a gas becomes liquid at a lower temperature than it’s normal boiling point.



History of gases. A British physicist named Robert Boyle, realized that gas is equivalent to the pressure if the temperature is sustained. This is the first law. The second law is the Charles Law. This law is named after a French physicist Jacques-A.-C.Charles. This law compares the volume of a gas to the temperature. However, the Charles law was discovered by English physicist John Dalton and French physicist Joseph Gay-Lussac in 1802. The combination of Boyle’s law, and Charles Law makes up the perfect-gas law.

Melting and boiling point of different gases. Freezing Point: Water: 0˚C or 32˚F, Hydrogen: -259.2˚C, tungsten: 3,370˚C, diamonds: above 3,5000˚C

Melting Point: Chlorine: -35˚C, Ether: 35˚C, Helium: -269˚C, Hydrogen: -253˚C, Oxygen: -83˚C, and Water: 100˚C

How does Pressure affect Gas?
==**Pressure affects gas by making its molecules move constantly trying to escape, or some times the gas changes. An example would be a liquid sealed in a container going through evaporation and turning into a gas.**==

How gas reacts under pressure?
==**When gas is under pressure its molecules are moving frequently (non-stop) trying to escape whatever it is shut up inside. An Example would be: Gas trapped inside a container, its molecules hitting the sides of the container trying to escape.**==



Research Citations:


 * States of Matter. (2012). In States of Matter. Retrieved January 25, 2012, from Expert Space http://expertspace.grolier.com/article?id=10001990&product_id=ngo
 * Yeaple, F. D. (2012). Gases in Industry. In The New Book of Knowledge. Retrieved January 25, 2012, from Grolier Online http://nbk.grolier.com/article?id=a2011420-h&product_id=nbk
 * Ehrenberg, W. (2012). Gas. In Encyclopedia Americana. Retrieved January 30, 2012, from Grolier Online http://ea.grolier.com/article?id=0171550-00&product_id=ea
 * Sebera, D. K. (2012). Boiling. In Encyclopedia Americana. Retrieved January 30, 2012, from Grolier Online http://ea.grolier.com/article?id=0052660-00&product_id=ea


 * "Gas Chromatography." //Sheffield Hallam University//. N.p., N.d. Web. 30 Jan. 2012. <[|__http://teaching.shu.ac.uk/hwb/chemistry/tutorials/chrom/gaschrm.htm__]>.
 * Lower, Stephen. "Observable Properties Of Gas." //General Chemistry virtual textbook//. N.p., 2004-2011. Web. 30 Jan. 2012. <[|__http://school.nettrekker.com/goExternal?np=/external.ftl&pp=/error.ftl&evlCode=302795&productName=school&HOMEPAGE=M__]>
 * Benson, Tom . "Gas Pressure." //NASA//. N.p., 30 July 2010. Web. 30 Jan. 2012. <[|__http://www.grc.nasa.gov/WWW/k-12/airplane/pressure.html__]>.

Image Citations:


 * //Hydrogen//. 2011. //The Element Hydrogen: Simplest Element in the Universe//. Web. 1 Feb. 2012. .
 * Benson, Tom . "Gas Pressure." //NASA//. N.p., 30 July 2010. Web. 30 Jan. 2012. <[|__http://www.grc.nasa.gov/WWW/k-12/airplane/pressure.html__]>.
 * //Expansion of a Gas//. //Chem 201 - 3. The Second Law//. Web. 8 Jan. 2012. <http://www.google.com/imgres?q=gas+molecules+expanding&um=1&hl=en&safe=active&sa=N&tbm=isch&tbnid=S8szz6bZpjp55M:&imgrefurl=http://www.chem.brown.edu/research/crp/Edu/Documents/00_Chem201/3_second_law/3-second_law-frames.htm&docid=GVIVE2sdj83pkM&imgurl=http://www.chem.brown.edu/research/crp/Edu/Documents/00_Chem201/images/Expansion_of_a_Gas.gif&w=720&h=540&ei=UVwyT5G6Mcfqtgfmx_WGBw&zoom=1&iact=hc&vpx=544&vpy=151&dur=1872&hovh=194&hovw=259&tx=156&ty=119&sig=107121474456983215566&page=1&tbnh=138&tbnw=184&start=0&ndsp=9&ved=1t:429,r:2,s:0&biw=990&bih=497>.