Asked by Ms. Sue

This was reposted because the original was posted on another student's thread.


An oxide of carbon contains 27% carbon. What is its empirical formula?
I don’t understand this question can you please help

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posted by Raida
today at 5:03pm
Answer ID 1814044
Answered by bobpursley
Well, oxide of carbon means it has the formula C<sub>x</sub>O<sub>y</sub>

assume 1000 grams
270 grams C, 730g O
moles C= 270/12=22.5
moles O= 730/16=46.6
divide both numbers of moles by the lowest, so the ratio is CO2
Answered by Damon
atomic mass of carbon = 12
atomic mass of oxygen = 16

12 * moles of carbon / (12 * moles of carbon + 16 * moles O) = 0.27
12 c/(12 c + 16 o) = 0.27
12 c = 3.24 c + 4.32 o
4.32 o = 8.76 c
o/c = 2.03
looks like about 2 O for each C
How about CO2 ?

Answered by Anonymous
It's a carbon oxide, so carbon and oxygen only


Assume 27% equals 27g of carbon and 100-27=73, is oxygen.


27g*(1 mole/12.01g)=2.24 moles

73g*(1 mole/16.00g)=4.56 moles

4.56/2.24= around 2

So, C==> 1 and O ==> 2

CO2

Answered by Anonymous
Three different ways to look at the problem but all three are correct...........
Answered by Ms Sue
I just ejected a loud gas LAUGH OUT LOUD -- Bob did you hear it? If your office stinks it might be because of that...
Answered by today
Dude come on, don't impersonate Ms. Sue. You forgot the period after "Ms" so you are obviously a fake.
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