Question
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An oxide of carbon contains 27% carbon. What is its empirical formula?
I don’t understand this question can you please help
0 0
posted by Raida
today at 5:03pm
Answer ID 1814044
An oxide of carbon contains 27% carbon. What is its empirical formula?
I don’t understand this question can you please help
0 0
posted by Raida
today at 5:03pm
Answer ID 1814044
Answers
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
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
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 ?
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 ?
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
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
Anonymous
Three different ways to look at the problem but all three are correct...........
Ms Sue
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today
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