Asked by Selena
Combustion analysis of 0.300 g of an unknown compound containing carbon, hydrogen, and oxygen produced 0.5213 g of CO2 and 0.2835 g of H2O. What is the empirical formula of the compound?
C2H5O
C3H8O2
C2H10O3
C2H5O2
C2H5O
C3H8O2
C2H10O3
C2H5O2
Answers
Answered by
DrBob222
Convert g CO2 to percent C.
Convert g H2O to percent H.
Add %C and %H and subtract the sum from 100 to obtain %O.
Then take 100 g sample which will give you the percents in grams.
Convert gC, gH, and gO to moles. Then find the ratio of each element to the smallest in whole numbers.
Post your work if you get stuck.
Convert g H2O to percent H.
Add %C and %H and subtract the sum from 100 to obtain %O.
Then take 100 g sample which will give you the percents in grams.
Convert gC, gH, and gO to moles. Then find the ratio of each element to the smallest in whole numbers.
Post your work if you get stuck.
Answered by
TutorCat
http://preparatorychemistry.com/Bishop_Combustion_Analysis.htm
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