Elbow it!!!, Really fun :) Options

[Hell-Rell]

aight you play this game by typin a word or sentence with your elbows! the user above give you


I'll start the word off


cookies

[*salcha*]

Acetone, Propylene Carbonate, Dimethyl Glutarate, Dimethyl Succinate, Dimethyl Adipate, Tocopheryl Acetate, Panthenol

1. Acetone:

Acetone is a colorless mobile flammable liquid with melting point at -95.4 °C and boiling point at 56.53 °C. It has a relative density of 0.819 (at 0 °C). It is readily soluble in water, ethanol, ether, etc., and itself serves as an important solvent. The most familiar household use of acetone is as the active ingredient in nail polish remover. Acetone is also used to make plastic, fibers, drugs, and other chemicals.

Source: http://en.wikipedia.org/wiki/Acetone

Acetone is a colorless, flammable, and volatile liquid with a characteristic odor that can be detected at very low concentrations. It is used in consumer goods such as nail polish remover, model airplane glue, lacquers, and paints. Industrially, it is used mainly as a solvent and an ingredient to make other chemicals.
Acetone is the common name for the simplest of the ketones. The formula of acetone is CH3 CO CH3.
The International Union of Pure and Applied Chemistry's (IUPAC) systematic name for acetone is 2-propanone; it is also called dimethyl ketone. The molecular weight is 58.08. Its boiling point is 133°F (56°C) and the melting point is -139.63°F (-95.4°C). The specific gravity is .7899.
Acetone is the simplest and most important of the ketones. It is a polar organic solvent and therefore dissolves a wide variety of substances. It has low chemical reactivity. These traits, and its relatively low cost, make it the solvent of choice for many processes. About 25% of the acetone produced is used directly as a solvent.
About 20% is used in the manufacture of methyl methacrylate to make plastics such as acrylic plastic, which can be used in place of glass. Another 20% is used to manufacture methyl isobutyl ketone, which serves as a solvent in surface coatings. Acetone is important in the manufacture of artificial fibers,explosives, and polycarbonate resins.
Because of its importance as a solvent and as a starting material for so many chemical processes, acetone is produced in the United States in great quantities. In 1999, the worldwide acetone market reached 9.4 billion lb (4.27 billion kg) at a steady growth rate of 2-3% per year. Acetone is prepared by several routes, from petrochemical sources. The methods of its synthesis include oxidation of 2-propanol (isopropyl alcohol), the hydration of propene, and as a co-product (with phenol) of the O2-oxidation of cumene.
Acetone is normally present in low concentrations in human blood and urine. Diabetic patients produce it in larger amounts. Sometimes "acetone breath" is detected on the breath of diabetics by others and wrongly attributed to the drinking of liquor. If acetone is splashed in the eyes, irritation or damage to the cornea will result. Excessive breathing of fumes causes headache, weariness, and irritation of the nose and throat. Drying results from contact with the skin.
Source: http://www.bookrags.com/sciences/chemistry/acetone-woc.html

I am not sure what you mean by “desired properties”. So what I will do is
describe the molecular structure of acetone and relate that to the most
common
usage of acetone.

For those who are not familiar with the molecular geometry and chemical
structure of acetone, imagine a threebladed airplane propeller. At the
center
of this propeller there is a carbon atom. The three blades of the propeller
are the bonds from the carbon atom. At the tip of one of the blades we
find an
oxygen atom. At the other two blades’ tips we find a CH3 group (for our
purposes, we can just imagine these as carbon atoms as well).

Since two of the propeller blades are made up of carbontocarbon bonds (a
carbon is at the tip of the blade and bonded to the central carbon), these
two
blades are essentially nonpolar. The third blade, however, is representative
of a carbontooxygen bond (it is actually a doublebond, but that is not
important right now). We know that oxygen is far more electronegative than
carbon, that is, oxygen is better at attracting the pairs of electrons that
form bonds between the central carbon and the oxygen. We can therefore
imagine
that the electrons spend a lot more time near the oxygen than near the
carbon.
Since electrons are negatively charged, the oxygen becomes partially negative
relative to the central carbon. We say that bond is polar, and, since
there is
no other polar bond within the acetone structure that could cancel out this
polarity, we say that the molecule has a netdipole. Just like a magnet, it
can be very good at attracting other molecules with a netdipole.

A lot of the chemical and physical properties of acetone can be traced
back to
the presence of this netdipole within its geometry. For example, acetone has
a higher boiling point than other molecules with similar masses to acetone
but
which do not have the netdipole. It dissolves very well in water because
water also acts like a polar molecule. It is a good solvent for a wide
range of
organic compounds, because most of these compounds have some polarity as well.

The chemical reactions of acetone are also dependent on this carbontooxygen
bond. Most compounds that react with acetone will either have a positive
functionality that tends to be attracted to the negative site found in the
oxygen, or a negative functionality that tends to be attracted to the
positive
site found in the carbon.

I hope that helps.
R. Gregorious
====================================================
I found searching Google for "flame temperatures" I found a nice little
table:
http://www.engineeringtoolbox.com/9_422.html .

They are more like 1900C for fuel pre-mixed with air.
Pre-mixed is what a Bunsen burner does, and your gas stove, too.

There is not really very much variation, they are all around1950C.
Hydrogen about 2050C.
Acetylene with 2400C is exceptional. (Isn't an alkane, admittedly.)
I have not yet guessed how you got your 1300C number.

More scatter, but lots of references, at:
http://hypertextbook.com/facts/1998/JamesDanyluk.shtml

It is likely a diffusion-flame can have a lower temperature than a
pre-mixed flame.
But it would not really be a constant of the gas,
it would be an effect of a particular geometry of flame,
loosing heat in all directions about as fast as it can make that heat.
A larger diffusion flame, perhaps partly occupied by hot crumbs of rock to
obstruct heat-radiation,
would burn hotter inside.
Eventually you have re-invented some ancient-style pottery furnace,
and it might approach the temperature of a pre-mixed flame.

The alternatives are "pre-mixed" or "diffusion-flame"
(in addition to choosing between air and pure oxygen, of course).

A diffusion flame is like a candle flame. Fuel gas on the inside, air on
the outside,
diffusing through each other as fast as they can so they can react.
Not really very fast. A diffusion flame "drifts" upwards by
gravity/convection.

A pre-mixed flame is a jet of dangerously mixed cool gas going one way,
and a flame front racing the other way (upstream) as fast as it can.
There is a narrow point in the nozzle where the gas flows faster than the
flame can propagate,
then the flow spreads out and slows down.
That is why the flame front can stand still before your eyes.
It is the round bottom of the little blue flame in your gas stove top burner.
The gasses burn near-instantly as they cross the "flame front".
Suddenly the gasses reach their ideal maximum temperature, then they start
cooling down as they flow away.
You therefore have a small place where the torch-flame has not yet cooled
down by any significant amount.

If the distinction is not clear to you, think about the three components
required for fire -
fuel, oxidizer, and heat.
If you mix fuel and oxidizer first, then add heat, that is pre-mixed.
If you heat fuel and/or air first, then mix, it will be a diffusion-flame.
When the fuel and oxidizer enter the hot zone by different paths, it must
be a diffusion-flame.

hope that helps-
Jim Swenson


Source: http://www.newton.dep.anl.gov/askasci/chem03/chem03356.htm









You better type the whole thing.