in chemistry, what exactly is a mole?

Answer 1

The amount of a substance that contains as many atoms, molecules, ions, or other elementary units as the number of atoms in 0.012 kilogram of carbon 12. The number is 6.0225 × 1023, or Avogadro's number. Also called gram molecule.
The mass in grams of this amount of a substance, numerically equal to the molecular weight of the substance. Also called gram-molecular weight. See table at measurement.

Basically its a measurement of atoms that can be used for any substance.... I think

Answer 2

It is simply just like this....


What is a Mole?

A mole is the amount of pure substance containing the same number of chemical units as there are atoms in exactly 12 grams of carbon-12 (i.e., 6.023 X 1023). This involves the acceptance of two dictates -- the scale of atomic masses and the magnitude of the gram. Both have been established by international agreement. Formerly, the connotation of "mole" was "gram molecular weight." Current usage tends to apply the term "mole" to an amount containing Avogadro's number of whatever units are being considered. Thus, it is possible to have a mole of atoms, ions, radicals, electrons, or quanta. This usage makes unnecessary such terms as "gram-atom," "gram-formula weight," etc.

All stoichiometry essentially is based on the evaluation of the number of moles of substance. The most common involves the measurement of mass. Thus 25.000 grams of water will contain 25.000/18.015 moles of water, 25.000 grams of sodium will contain 25.000/22.990 moles of sodium.

The convenient measurements on gases are pressure, volume, and temperature. Use of the ideal gas law constant R allows direct calculation of the number of moles: n=P V/R T. T is the absolute temperature, R must be chosen in units appropriate for P, V, and T. The acceptance of Avogadro's law is inherent in this calculation; so too are approximations of the ideal gas.

Answer 3

The mole is a measure of amount of a substance (actually a measure of the number of component units). 1 mole is equal to 6.022*10^23 units, defined as the number of carbon 12 atoms there are in 12g of carbon 12.

Answer 4

A mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 12 grams of carbon 12, where the carbon 12 atoms are unbound, at rest and in their ground state.[1] The number of atoms in 12 grams (or, 0.012 kilograms) of carbon 12 is known as Avogadro's number. The currently accepted value is 6.022 1415(10) × 1023 (2002 CODATA).

A mole is a dimensionless name for a number, much like dozen or googol.

The relationship of the atomic mass unit to Avogadro's number means that a mole can also be defined as: That quantity of a substance whose mass in grams is the same as its atomic weight. For example, iron has an atomic weight of 55.845, so a mole of iron weighs 55.845 grams. This notation is very commonly used by chemists and physicists.

However, most chemical engineers as well as many other engineers and scientists differentiate between gram moles and kilogram moles (kgmol or kmol): 55.845 grams in a gram mole of iron and 55.845 kilograms in a kilogram mole of iron. Similarly, engineers and scientists in the United States use the pound mole (lbmol): 55.845 pounds in a pound mole of iron.

Answer 5

A mole is a way to measure a great amount of atoms/compounds/molecules and such by weight. The equation is 6.02252 x 10 to the 23rd power. To find moles for a specific element you just look at the atomic weight.
For example, Carbon's atomic weight is 12.011, therefore one mole of Carbon would be 12.011 grams.
If you wanted to find the weight of a mole of a molecule you would take the atomic weights of both elements and add them together.
More than one mole, just multiply. Example, if you wanted three moles of Carbon you would multiply 12.011 by three.
Six moles of NaSO would be 6 x (Na + S + O)

Answer 6

Remove Your Moles, Warts & Skin Tags in 3 Days
Easily, Naturally And Without Surgery

Answer 7

You can use Avagadro's number as a reference to a mole for any element. This number is 6.02 x 10^23 atoms. This is just an average number that some chemist named avagadro came up with. Hence the weight of a mole is = (Atomic Mass) x (Avagadro's #).

Answer 8

Quoting: "Mole (unit), also mol, is the SI unit used in chemistry for an amount of a particular object based on Avogadro's number, approximately 6.02252 × 1023."

Answer 9

Moles were defined to solve the problem of counting large numbers of molecules. With moles, you count the number of molecules in the sample by weighing it.
Learn to convert between moles and molecules, and moles and grams.

Using moles to count molecules. A mole of any substance is 6.02×1023 molecules of that substance. You can use this as a conversion factor to turn moles into molecules. For example, to figure out how many molecules there are in 0.001 moles of water,

Answer 10

mole is a measurement -how many atoms/molecules/ions/particles/objects you have

when u have 12 eggs , u say 'i have a DOZEN eggs'

when u have 6 × 10^23 eggs, u say 'i have a MOLE eggs'

hope this helps