Dont worry, I also had a lot of difficulties withat first.

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First things first; pull the end your PeriodicTable. uncover the atomic weight (probably inthe top left corner.) This Atomic weight isthe weight of 1 mole of atoms of the kind. For circumstances look at N (Nitrogen), you will seethe atomic mass is 14.00674 grams. So that meansif you had actually 1 mole of nitrogen atoms, it wouldweight, 14.00674 grams.

So if you have actually a fraction of a mole, speak forinstance, simply multiply * 14.00674 grams toobtain the weight, 7.00337 grams. (I used theequation below):

Fraction that a mole * Atomic weight = weightor mass girlfriend have

Now we have to obtain what portion of a mole youhave. Come start, girlfriend need know that all a molemeans is you have 6.022 x 1023 atoms ofthat type. so if i tell you I have a mole ofnitrogen, climate I have 6.022 x1023nitrogen atoms. The ugly number is calledAvogadro"s Constant, NA. Scientist usage NAjust for this reason they don"t need to keep writing that longnumber over and over again.

To gain the portion of a mole girlfriend have, takethe variety of atoms friend have, and divide the by6.022 x 1023. (Use equation below):

Number of atoms you have / 6.022 x1023 = portion of a mole

After you do that, plug it right into the an initial aboveequation and also that should give you her answer.

1 mole = 6.03 x 1023 particles.One mole of any element has a fixed in gramsthat is same to its atom number, and hasexactly 6.02 x 1023 atoms - howeverbecause the atoms of each aspect have differentsizes and also weights, climate the volume the each oneoccupies is different. Also, some aspects aresolids, liquids, or gases in ~ room temperature, sothey will additionally occupy various volumes.

The trick come working with moles is tounderstand the you are dealing with differentunits, and also you need to translate between them.We contact this "units factoring" due to the fact that itinvolves setting up ratios the the units andcancelling... For example: money. The smallestamount that money you can have is a penny. Youcan"t have fifty percent a penny. Yet you have the right to translateevery lot of money right into its identical numberof pennies. The conventional is that 1 dissension = 100pennies. So, 10 dollars = 10 dollars x 100pennies/dollar = 1000 pennies. Similarly, fifty percent adollar = 0.5 dissension x 100 pennies/dollar = 50pennies. And, functioning backwards, if someonegives you 50 pennies and also asks you how countless dollarsyou have, you deserve to probably execute this in your head,but let"s write it the end for the sake ofillustrating the point:

50 pennies x 1 dollar/100 pennies = 50/100 =0.5 dollar. The works as with this because that doingmole portion problems.

If one mole the carbon, for example, has actually a massof 12 grams, climate 12 grams that carbon contain(12)(6.03 x 1023 ) atoms. Just how manyatoms are in 3 grams that carbon? Well... (3grams that carbon) x (1 mole of carbon/12 grams ) =3/12 = 1/4 of a mole of carbon.

Then... ( 1/4 the a mole) x (6.02 x1023 atoms/mole) = approximately 1.5 x1023 atoms. If you have a compoundlike H2O, then:

one mole of water consists of 6.02 x1023 molecules of water. but eachmolecule the water consists of 2 H and 1 O atom = 3atoms, so there are about 1.8 x1024 atoms in a mole the water.

In having trouble v the id of what a moleis and how to use the concept, you room not alone.Many civilization have difficulties understanding what amole is. A mole is a cumulative term. simply asone says, a bunch that grapes, a proud of lions, orbetter still, a dozen cookies, one can say, a"mole of atoms", or a "mole that molecules". A moleis a arsenal of Avogadro number of things. Thethings can be atoms or molecules.They couldalso be horses. A mole of steeds would be Avogadronumber of equines (a lot actually !). Avogadronumber is 6.023 x 10(23).

A mole that H (hydrogen) atomscontains 6.023 x 10(23) H atoms. A moleof H2molecules has 6.023 x 10(23)H2 molecule or2 moles of H atom (since every molecules has 2atoms).

A mole that CaCO3 (calcium carbonate) hasone mole (Avogadro number) of Ca atoms, one moleof C atoms and 3 moles of O atoms.

so what isspecial around the Avogadro number. It isjust asimple multiplicative constant that relates atomicweights come the simpler, more familiar measure up ofthe gram(g).

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Look up a regular table that theelements. Under each element entry, girlfriend willusually find the atomic mass. Because that example,underOxygen, you find the atomic weight is 16.00. Thismeans the 16.00 g of oxygen has actually Avogadro numberof oxygen atoms. Carbon is 12.01. So a 12.01 gsample that carbon has Avogadro variety of carbonatoms. If us take the CaCO3 example, theformula load is the amount of the atomic masses. Wefind that for CaCO3, the formula load is:

Ca(40.08) + C (12.01) + 3 O (16.00) = 100.1

100.1 gof CaCO3 is one mole ofCaCO3. We deserve to prepare itby reaction, one mole the CaO weighing 56.08 g, withone mole of CO2 weighing 44.01 g. If wepreferred towork with ounces, instead of g, and wished torelated the atomic load to ounces, climate thevalue that us would decided for the Avogadro numberwould it is in different.