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

You are watching: How many atoms are in three moles of carbon?

First points first; pull the end your PeriodicTable. discover the atomic weight (probably inthe height left corner.) **This Atomic load isthe load of 1 mole of atoms of that kind.** For circumstances look in ~ N (Nitrogen), you will seethe atom mass is 14.00674 grams. So the meansif you had 1 mole the nitrogen atoms, the wouldweight, 14.00674 grams.

So if you have a fraction of a mole, say forinstance, just multiply * 14.00674 grams toobtain the weight, 7.00337 grams. (I provided theequation below):

**Fraction that a mole * Atomic load = weightor mass you have**

Now we have to obtain what portion of a mole youhave. Come start, friend need know that **all a molemeans is you have actually 6.022 x 1023 atoms ofthat type.** so if ns tell friend I have a mole ofnitrogen, climate I have actually 6.022 x1023nitrogen atoms. That ugly number is called**Avogadro"s Constant, NA.** Scientist usage NAjust therefore they don"t need to keep writing that longnumber over and also over again.

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

**Number of atom you have actually / 6.022 x1023 = fraction of a mole**

After you carry out that, plug it right into the very first aboveequation and that should provide you your answer.

**Answer 2:**

**1 mole = 6.03 x 1023 particles.One mole of any type of element has actually a fixed in gramsthat is equal to its atomic number, and also hasexactly 6.02 x 1023 atoms** - howeverbecause the atoms of each element have differentsizes and also weights, then the volume that each oneoccupies is different. Also, some elements aresolids, liquids, or gases in ~ room temperature, sothey will also occupy different volumes.

The trick to working v moles is tounderstand the you are dealing with **differentunits**, and you need to translate between them.We speak to this **"units factoring"** due to the fact that itinvolves setting up ratios the the devices andcancelling... Because that example: money. The smallestamount the money you have the right to have is a penny. Youcan"t have fifty percent a penny. But you can translateevery lot of money into its identical numberof pennies. The traditional is the 1 dissension = 100pennies. So, 10 dollars = 10 dollars x 100pennies/dollar = 1000 pennies. Similarly, half adollar = 0.5 dollar x 100 pennies/dollar = 50pennies. And, working backwards, if someonegives you 50 pennies and also asks friend how countless dollarsyou have, you have the right to probably do this in her head,but let"s compose it the end for the services ofillustrating the point:

50 pennies x 1 dollar/100 pennies = 50/100 =0.5 dollar. It works similar to this because that doingmole fraction problems.

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

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

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

**Answer 3:**

**In having actually trouble with the id of what a moleis and how to use the concept, you are not alone.Many human being have troubles understanding what amole is. A mole is a collective term.** just asone says, a bunch the grapes, a proud of lions, orbetter still, a dozen cookies, one might say, a"mole that atoms", or a "mole of molecules". **A moleis a arsenal of Avogadro variety of things.** Thethings could be **atoms or molecules.****They couldalso be horses. A mole of horses would it is in 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 includes 6.023 x 10(23)H2 molecule or2 mole of H atoms (since each molecules has actually 2atoms).

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

for this reason what isspecial around the Avogadro number. **It isjust asimple multiplicative constant that relates atomicweights to the simpler, an ext familiar measure ofthe gram(g).See more: Which Elements Can Form Diatomic Molecules Joined By A Single Covalent Bond?**

Look up a periodic table the theelements. Under each aspect entry, you willusually uncover the **atomic mass**. Because that example,underOxygen, you find the atomic load is 16.00. Thismeans that 16.00 g that oxygen has Avogadro numberof oxygen atoms. Carbon is 12.01. So a 12.01 gsample the carbon has Avogadro variety of carbonatoms. If us take the CaCO3 example, theformula load is the amount of the atomic masses. Wefind the 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 can prepare itby reaction, one mole of CaO weighing 56.08 g, withone mole of CO2 weighing 44.01 g. If wepreferred towork with ounces, instead of g, and also wished torelated the atomic load to ounces, then thevalue that us would determined for the Avogadro numberwould be different.