Clarification

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magaliolide1D
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Joined: Thu Jul 11, 2019 12:15 am

Clarification

Postby magaliolide1D » Thu Oct 03, 2019 6:01 pm

Do you always go from empirical to molecular? Could you go from molecular to empirical and is that something that occurs? Also if that is a thing, why would from molecular to empirical?

Ali Polansky 1A
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Re: Clarification

Postby Ali Polansky 1A » Thu Oct 03, 2019 6:17 pm

You can find the empirical formula from the molecular by simplifying the ratio. For example, IF the molecular formula was Os3C12O12, the ratio 3:12:12 can be simplified to 1:4:4, so the empirical formula would be OsC4O4

Vivianvelazquez_1J
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Re: Clarification

Postby Vivianvelazquez_1J » Thu Oct 03, 2019 6:18 pm

I'm sure you can go from molecular back to empirical but I'm not sure if you'll ever have to do it. If you do you would need all of the factors including obviously the actual compound that you're converting, the ratio, the molecular mass when it's at its highest and the molecular mass of the compound it self so you could work backwards.

Venus_Hagan 2L
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Joined: Fri Aug 02, 2019 12:16 am

Re: Clarification

Postby Venus_Hagan 2L » Thu Oct 03, 2019 7:42 pm

It is possible to go from molecular to empirical. You would just need to get each of the subscripts in the formula and change it so they are at the simplest ratio and still keeping whole numbers. I don't think we would really need to do this though.

TimVintsDis4L
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Joined: Sat Aug 17, 2019 12:17 am

Re: Clarification

Postby TimVintsDis4L » Thu Oct 03, 2019 8:10 pm

I'm fairly certain that you can find both if we are given enough information. It's just like how we can find the mass of sample, the number of moles, and the molar mass of the element if we are given at least 2 of these.

Alexandra Bartolome 2H
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Joined: Sat Jul 20, 2019 12:17 am

Re: Clarification

Postby Alexandra Bartolome 2H » Thu Oct 03, 2019 9:38 pm

Venus Hagan 3D wrote:It is possible to go from molecular to empirical. You would just need to get each of the subscripts in the formula and change it so they are at the simplest ratio and still keeping whole numbers. I don't think we would really need to do this though.


I think you meant to say that the coefficients in the chemical equation need to be at its simplest ratio to go from the molecular to empirical formula. You are not supposed to change the subscripts in a chemical equation because they indicate the number of atoms of an element present in chemical formulas.

Jake Gallardo 3G
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Joined: Wed Sep 18, 2019 12:18 am

Re: Clarification

Postby Jake Gallardo 3G » Thu Oct 03, 2019 9:40 pm

Both should work, but it heavily depends on the information given.


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