Some one want to explain Moles to me?

Question

I know this is a bit elementary, and i love chemistry and im only just starting it. Would someone care to give a straightfoward explaination of a mole and how we use them in chem with examples with different elements? Thank you.

Answer 1

mole is defined as the quantity of a substance that has the same number of quantity as are found in 12 grams of carbon 12,this number is called Avogadro's Number: 6.022x10*23. it is used in chemistry because it gives a consistent method to convert between atoms/molecules and grams.
EX: you want to figure out how many molecules there are in 0.001 moles of water:
0.001 moles H2O x 6.02x10*23 water molecules/1mole water = 6.02x10*20 water molecules

EX: how many moles are there in 100 water molecules?
100 water molecules x 1mole water/ 6.02x10*23 water molecules =1.66x10*-22 moles water

EX: H2O has a molecular weight of 18.0 (16 for hydrogen and 1 for each O), determine the mole-to-gram relation for water

1mole water= 18grams water

how many moles are there in 100grams of water?
100 grams H2O x 1mole H2O/ 18grams H2O= 5.56moles H2O

how many grams are there in 6moles of O2:

6.0 moles O2 x 32 grams O2/ 1mole O2= 192grams O2

Answer 2

A mole is a unit of quantity. Think of it as the same concept as a dozen.

A dozen is 12 of anything. Well, a mole is 6.022 x 10^(23) of anything. This is also known as Avogadro's number.

So a dozen flowers or a mole of flowers. Pick a dozen, you do not have a house big enough.

You can have a mole of dollars (by the way, there are not enough dollars in the world to make a mole of dollars).

You can have a mole of sand grains. and so on.

In chemistry, for example, a mole of carbon atoms is, you guessed it, 6.022 x 10^23 atoms.

If we measure the weight of one carbon atom and multiply by Avogadro's number, we obtain the weight of one mole of carbon atoms.

By convention this is also called the atomic (or molecular) weight and is expressed in units of gram / mol, e.g. how many grams a mol of the stuff weights

So instead of doing all the calculations on an atom by atom basis we do chemical calculations with a large number of atoms, 6.022 x 10^23 to be exact (1 mole).

Answer 3

A mole is Avogadro's number (6.02 x 10^23) of anything. Personally, I'd like to have a mole of dollar bills.

Moles are a convenient way of relating elements and compounds.

If you can measure the mass of a compound, simply divide the mass by it's molecular weight to determine how many moles of it you have. Then, knowing how many moles of the compound you have, you also know how many moles of each of the atoms that make up that compound you have.

Knowing this information helps you determine how reactions between compounds will take place. When you learn about stoichiometry, you'll know what I mean.

Have fun with your chemistry.

Answer 4

Look... a mole is just a unit. Like a meter or a furlong. Only this one is usually used to count the number of atoms.

Atoms, of course, are so ridiculously small that just about anything you want to talk about is going to have a ridiculously large number of them. And that's where moles come in. It is reasonable that you can hold a couple moles of atoms in your hand. Moles are a nice way of bridging between something we can measure (like grams) and something we can't (like number of atoms), and all we need to know is molecular mass to make up the difference!

Nor does it have to be just atoms. For example, there have been 0.7 moles of nanoseconds in the history of the universe. The observable part of the universe contains about 0.11 moles of stars. Or, if you have a mechanical pencil, about 474 0.5 mm leads are needed to have a mole of carbon atoms (where I buy them, that's about a box and a half... I sometimes buy several moles at a time, but I don't tell the cashiers unless I want them to get funny looks on their faces).

One mole is 6.022 x10^23 of something. LOTS!

Answer 5

1 mole = 6.022115 x 10 23 things. We use it in chem to approximate the number of atoms in saples we can actually handle. For example, 1 mole of carbon is 12 grams of carbon, or about twenty mechanical pencil leads. You may notice that the mass of 1 mole of carbon is also its atomic number. This holds constant for all elements- the mass of a mole of an element is its atomic mass written in grams.

Answer 6

A mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon-12, where the carbon-12 atoms are unbound, at rest and in their ground state.The number of atoms in 0.012 kilogram of carbon-12 is known as Avogadro's number, and is determined empirically. The currently accepted value is 6.0221415(10)×1023 mol-1

Answer 7

A mole of a substance is an amount wherein there are 6.02 x 10^23 molecules or atoms of that substance. An element's molecular weight is one mole of that substance. 12.0 grams of Carbon is one mole of carbon. 18 grams of water is one mole of water, etc. Moles are used to balance reactions, to determine molarity (concentration) of solutions, among others.

Answer 8

Mole is the unit used to count atoms or molecules in chemistry and it equal avogadros number of atoms or molecules ,, 1 mole of Na (sodium) element equal about 22.9 grams of sodium were the 22.9 is the atomic mass of sodium,, 1 mole of NaCl molecules equal 22.9 +35.45 = 58 grams of sodium chloride

Answer 9

a mole is a certain set number of particles, so a mole of helium atoms will weigh less than a mole of iron atoms;the ratios of atoms in a molecule can be deduced from the weights of the materials...................