Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: tou on February 11, 2008, 03:57:55 PM
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Hi
I don't know how to get the correct answer, I've tried but I failed to answer the question.
Question: When you consume 1.00g of vitamin C, how many oxygen atoms are you eating?
Vitamin C: C6H8O6
The answer: 2.05 x 1022
Thank you very much!
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First of all you should show you at least tried.
But I will give you a start: first calculate how many moles of vitamin C you have in 1.00 gram
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Nr. of moles in vitamin C: 5.68 x 10-3
Then I thought, I should calculate the number of particles, thus the nr. of moles x 6.02 x 1023.
That is: 3.41 x 1021
Thus 1g of vitamin C contains 3.41 x 1021 particles/atoms.
Now I am not sure what the next step is...
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Almost there :)
Look at the formula - how many atoms of oxygen per 1 molecule?
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Aha... 3.41 x 6 = 2.05 x 1022
Now I wonder why I wasn't able to do it before, ::) :)
Thank you!