Question

2. In a molecule represented by the chemical formula C6H12O6, how many atoms of each element are present?

Answer 1

C6H12O6 is sugar. there are 6 of C (carbon atoms), 12 of H (hydrogen atoms), 6 of O (oxygen atoms)

Answer 2

the answers are in "C6H12O6" itself

Answer 3

The subscript beside each element indicates the number of atoms that are present to form a single molecule/compound of the substance. So, for C6H1O6, we have C, H and O. Hopefully you can see now the number of atoms present for each.

Answer 4

do you understand?

Answer 5

Each mole is equivalent to 1 atom of an element, am I right?(making sure)

Answer 6

If you're talking about one mole of a single atomic species, this would be a sample of that substance which contained 6.022 x 10^23 (Avogadro's Number) atoms. The same would go for one mole of a compound, that would be a sample which contained Avogadro's number of single molecules of that compound, or a sample which had a mass equivalent to its relative molecular mass in grams.

Answer 7

one mole is equal to 6.02214179 x 10^23 atoms. for example, if you have one mole of Oxygen, you have 6.02214179 x 10^23 Oxygen atoms

Answer 8

@Ciarán95 also explained it very well.

Answer 9

In this case there is 6 oxygen atoms. Wouldn't that be the same as having 6 moles of oxygen? 6O and O6

Answer 10

@Mateaus
1 mole is not the same as 1 atom
1 mole = 6.022 x 10^23 atoms

If you had one mole of the aforementioned glucose compound (C6H12O6), then you would have 6.022 x 10^23 individual C6H12O6 molecules in that sample. However, each of these individual molecules contains 6 atoms of oxygen, so overall 1 mole of glucose would contain 6(6.022 x 10^23) atoms of O, which is 3.6132 x 10^24 atoms, approximately. Hope that helps!

Answer 11

no, it would not be the same. as I said, one mole is equal to 6.02214179 x 10^23 atoms. so 6 moles of oxygen would equal 36.138 x 1023 atoms.

Answer 12

again, @Ciarán95 has explained it very well. (good job!)

Answer 13

do you understand?

Answer 14

Yes, I think I do but I was wondering in the case of just one element in determining their amu or mass. if I have 1 mole of Oxygen, I would have only 16g. If I have 1 atom of Oxygen, wouldn't that be 16g as well?

Answer 15

The only difference is that a mole can take over a whole compound and make it 6.022x10^23 while an atoms if just one piece of the whole mole.

Answer 16

not exactly make it 6.022x10^23 but is like I have x(A+B+C) x is the mole and multiplies by the inside producing more atoms of the elements inside the parenthesis(compound).

Answer 17

so if I have 2 moles of (A2+B+C3) I would have 4atoms of A, 2atoms of B and 6atoms of C

Answer 18

but then if avogadro's number ends in atoms, doesn't that mean that each atom is equal as well to avogadro's number?

Answer 19

that's correct. moles = grams/molecular mass. so 1 mole of Oxygen would equal x grams/15.999 or 16g. (sorry for the very late response, I had to get up for a minute)

Answer 20

do you have a specific problem that you need help with or are you trying to understand it in general?

Answer 21

I have 4 atoms of A, 2 atoms of B and 6atoms of C. That would be the same if I had 4moles of A, 2moles of B and 6 moles of C in terms of finding their mass. Am I correct?

Answer 22

The only difference is that a mole can count as a whole compound while an atom is for one.

Answer 23

A mole functions similarly as a dozen. A dozen means 12 of something whereas a mole means 6.022E23 of something.

That something can be atoms, molecules, etc.

So I read one of your questions @Mateaus asking if 1 atom of O would weigh 16 grams just b/c 1 mole of O weighs 16 grams. The answer is no. You can calculate the weight of 1 O atom as follows:

1 O atom x (1 mol of O / 6.02E23 O atoms) x (16 grams O / 1 mol of O) = 2.66E-23 grams is what 1 O atom weighs

Answer 24

The coefficients in front of reactants or products in a reaction can represent either the # of atoms or molecules of reactants or products or moles. It wouldn't matter which one you choose b/c everything is proportional

Answer 25

coefficients can represent # of atoms (or molecules) or the # of moles*

Answer 26

I understand that now. is just that professors when they ask to find the mass for example of 2O5 = 10 oxygen *16 = 160g of O. I get confused by that

Answer 27

O5 doesn't exist but I see what you're saying

Answer 28

there is 2 moles of 5 atoms of oxygen. How come they end up being 160g if the atoms weight less.

Answer 29

O5 just as example

Answer 30

I guess they just want the coefficients to represent the # of moles so you would have 2 moles of "O5", so lets find the "molar" weight

2 moles of O5 x (80 g of O5 / 1 mol of O5) = 160 g of O5

Answer 31

if you made the coefficient 2 to represent the # of O5 molecules

Answer 32

O5 is not 5 atoms of O? How is 80g of O5 if atoms weight less?

Answer 33

then

2 molecules of O5 x (1 mol of O5 / 6.022E23 molecules of O5) x (80 g O5 / 1 mol of O5) = 2.66E-22 grams is what 2 molecules of O5 weigh

Answer 34

Uh the 5 in front of the O is a subscript right? If so, then that means there are 5 atoms of O in 1 molecule of O5

Answer 35

See you can use either the weight of 2 "moles" of O5 or 2 "molecules" of O5 in your calculations. It's just that you have to be consistent with that in the rest of the problem

Answer 36

using moles just makes the #'s nicer

Answer 37

1 MOLE of O5 is 80 grams, or in other words, 6.022E23 MOLECULES of O5 weigh 80 grams

Answer 38

You getting this?

Answer 39

How do you write then 5 atoms of O?

Answer 40

Look it's not proper to write 5 atoms of Oxygen as \[O _{5}\] or even as 5O b/c Oxygen exists as a diatomic molecule. So you would need to write 5 atoms of Oxygen as \[\frac{ 5 }{ 2 }O _{2}\]

Answer 41

This is simply b/c \[O _{5}\] or O by itself doesn't exist

Answer 42

The point is that 1 mole = 6.022E23 of atoms (or anything) thus 1 mole does NOT equal 1 atom (or anything else)

Answer 43

The coefficients in reactions can represent either moles (which is 6.022E23 # of atoms or molecules, depending on if the coefficient is in front of an atom or a molecule) or directly atoms or molecules (depending on if the coefficient is in front of an atom or molecule). When you solve for the weight, you can let the coefficient represent either moles or directly atoms (or molecules). It doesn't matter but what does matter is you stay consistent with your choice for the rest of the problem

Answer 44

That's all I can really say

Answer 45

I see. So if I am asked to find the mass of a certain element. I just use their molar mass unless I am asked to find the mass of the atom of an element(?)

Answer 46

The periodic table doesn't have any "masses" on it. It has "weights". If you want to find the atomic weight of an element, just look it up on the periodic table. For example, Hydrogen has an atomic weight of about 1 gram / 1 mole. This means that Hydrogen weighs 1 gram when you have 1 mole or 6.022E23 atoms of Hydrogen.

Answer 47

An element is just a "type" of atom. For example, I can have a jar full of 5 million Helium atoms, but that jar only has 1 element (1 type of atom)

Answer 48

Yes, but if I am asked to find the weight of oxygen molecules for example

Answer 49

Okay so diatomic oxygen is O2. Let's say you want to find how much 1 O2 molecule weighs (not 1 "mol" but just 1 "molecule")

1 O2 molecule x (2 O atoms / 1 O2 molecule) x (1 mole of O atoms / 6.022E23 O atoms) x (16 grams of O atoms / 1 mole of O atoms) = 5.31E-23 grams

Answer 50

so 1 O2 molecule weighs 5.31E-23 grams

Answer 51

How do I know or where do I look up to know how many atoms each element's molecule has? I didn't know oxygen's molecule had 2 atoms for example.

Answer 52

How much does 1 mole of O2 molecules weigh? Or equivalently, how much does 6.022E23 molecules of O2 weigh?

6.022E23 molecules of O2 x (5.31E-23 grams of O2 / 1 molecule of O2) = 32 grams of O2

Answer 53

At standard temperature (not too high or too cold), Oxygen is diatomic, meaning it's O2. There is a mnemonic of remembering what elements exist as diatomic molecules at standard temperature and this is what it is. BrINClHOF (pronounced as Brinklehoff). Bromine exists as Br2, Iodine exists as I2, Nitrogen exists as N2, Cl exists as Cl2, Hydrogen exists as H2, Oxygen exists as O2, and Fluorine exists as F2

Answer 54

You just look at the "sub"scripts in front of the element to figure out how many atoms of that element there are in a molecule

Answer 55

If you got more questions, I suggest you post your own question on OpenStudy so you can get insight from other people

Answer 56

I see, so if I am asked to find the weight of a molecule, then I have so find the weight of the atoms of the element. and in the case of moles, I just find the amu of the element times the moles of the element.

Answer 57

yes

Answer 58

Yeah I understand it now. Just clearing it out.

Answer 59

1 amu is the same as 1gram/1mole

Answer 60

So Hydrogen's weight is about 1 amu or about 1gram/1mole

Answer 61

just 1 atom of Hydrogen*

Answer 62

and 1 atom is 1mole/6.022x10^23 * the mole of the element's atom/1mole

Answer 63

Yes

Answer 64

the weight of the element's mole*

Answer 65

No you had it right before. The weight of an atom is the amu of the atom divided by 6.022E23

Answer 66

Ex with Hydrogen

1 atom of Hydrogen x (1 mole of Hydrogen / 6.022E23 atoms of Hydrogen) x (1 gram H / 1 mol of H) = 1/6.022E23 grams or 1.66E-24 grams.

Answer 67

1atom C *(1mole/6.022x10^23)*(amu of C/1mole)

Answer 68

Ex with Carbon

(1 atom C x 12 amu)/6.022E23 atoms of C = 1.99E-23 grams is what 1 atom of C weighs

Answer 69

Ya you got it

Answer 70

Ok, thanks you for having so much patience haha

Answer 71

just one correction, the "amu" you have in the numerator should be "grams" instead. The "gram/mole" together is what makes up an amu

Answer 72

np man

Answer 73

I have been doing chemistry using just math ignoring what was atoms or moles etc to the points I ended confused a lot of times.

Answer 74

Ya make sure you know what the numbers "mean"