Asked by rose
"empirical formulas"
combustion of a 0.255g compound conatining only C,H and O, yields 0.561g CO2 and 0.306g H2O. what is the empirical formula of the compound?
combustion of a 0.255g compound conatining only C,H and O, yields 0.561g CO2 and 0.306g H2O. what is the empirical formula of the compound?
Answers
Answered by
DrBob222
Convert g CO2 to g C.
Convert g 2P to g H.
0.255 - g C - g H = g O.
Convert g C, H, O, to mols.
Find the ratio.
Post your work if you get stuck.
Convert g 2P to g H.
0.255 - g C - g H = g O.
Convert g C, H, O, to mols.
Find the ratio.
Post your work if you get stuck.
Answered by
rose
umm... i need some help, sorry but how do you convert them?? my chem teacher isnt the best :(
Answered by
DrBob222
I made a typo. It should read covert g H2O to g H.
g CO2 = 0.561/molar mass CO2 = ?
1 mol C in 1 mol CO2, then g C = mols CO2 x molar mass C = about 0.153g C.
Same process for the others (but note there are two mol H in 1 mol H2O).
g CO2 = 0.561/molar mass CO2 = ?
1 mol C in 1 mol CO2, then g C = mols CO2 x molar mass C = about 0.153g C.
Same process for the others (but note there are two mol H in 1 mol H2O).
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