1 gram = 6.03 X 10 ^ 23 atoms? EK

[orthoboy]

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[rockclock]

1 g = 6.022 x 10^23 amu

 

[MShopes]

Okay, in the examkrackers chemistry book, it states that 1 gram is equal to 6.03 X 10 ^ 23 atoms. How is that so? I thought that 1 mole is equal to 6.03 X 10 ^ 23, and one mole is equal to the number of grams that contains that many atoms, or the number of grams that is equal to the atomic weight of the element. I just don't know how they said 1 gram = 6.03 X 10^23.

If someone can elaborate that'd be great. Thanks!

Where in EK does it state that? As the above poster said, EK clearly said in red bold that 1 g = 6.022 x 10^23 amu...and one atom of carbon is equal to 12 amu.

 

[orthoboy]

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[neurodoc]

1 g = 6.022 x 10^23 amu

This thread is confusing. 1 gram is a unit of mass. 1 gram of hydrogen molecules at STP and a gram of nitrogen molecules at STP have exactly the same mass but a different number of molecules. Instead of saying 1 g= Avogadro's Number, you should say the 1 g molecular weight (gmw)= Avogadro's number.

 

[MShopes]

Yes I'm sorry that's what I meant. Could you please describe that relationship?

1 g=6.022*10^23 amu
12 g (molecular weight) =6.022*10^23 atoms
1 atom=12 amu

since 1 g=6.022*10^23 amu, then 12 g=12*(6.022*10^23) amu

since 12 g=6.022*10^23 atoms, then 6.022*10^23 atoms=12* (6.022*10^23) amu, now if you cancel 6.022*10^23 in both sides, you get 1 atom=12 amu.

That is how the formula 1 atom=12 amu relate to the formula 1 g=6.022*10^23 amu.

 

[neurodoc]

since 1 g=6.022*10^23 amu, then 12 g=12*(6.022*10^23) amu

I understand what you are trying to say, but saying that 1 g=6.022*10^23 amu is not correct. 1 gram is simply 1 gram of matter, as I pointed out above. You should say that 1 gram molecular weight of an atomic or molecular substance (actually its mass if you want to be precise) consists of Avogadro's number of the pafrticles that make up this substance.

 

[MShopes]

I understand what you are trying to say, but saying that 1 g=6.022*10^23 amu is not correct. 1 gram is simply 1 gram of matter, as I pointed out above. You should say that 1 gram molecular weight of an atomic or molecular substance (actually its mass if you want to be precise) consists of Avogadro's number of the pafrticles that make up this substance.

You are right but sometimes when we be too precise and focus on details, we lose the big picture which is what the MCAT focuses on. So I tend to focus on the big picture but you are absolutely right.

 

[orthoboy]

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[Cruzerthebruzer]

So you're saying that 1 gram of a substance with a molecular weight of 1 g/mol contains 6.02X10^23 atoms? In other words one mole contains that many atoms?

Yes