A certain compound was found to have a molar mass of 60.095 g. A 1.705 g sample of this compound was burned in pure oxygen gas. The measured amount of CO2 produced was 3.746 g, while that of H2O was 2.044 g. No other products were produced in the reaction.
How many moles of carbon were in the original sample that underwent combustion ?
2007-04-11 12:37:18 · 3 answers · asked by garture 1 in Science & Mathematics ➔ Chemistry
3.746/44
2007-04-14 21:06:33 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
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2016-05-16 12:18:01 · answer #2 · answered by Anonymous · 0⤊ 0⤋
Many combustion reactions ensue with organic and organic compounds. a super form of the time they are saturated alkanes. the thank you to make certain the empirical formula for saturated alkanes is: C (n) H (2n+2) So if there have been 5 carbons, 5 could be your n and you will get 12 hydrogens. So then once you paintings out the mass for C5H12 you get approximately seventy two.106g ( 12(5) + a million(12) ) = seventy two.106g subsequently, interior the top, your empirical formula is C5H12
2016-12-09 00:36:26 · answer #3 · answered by ? 4 · 0⤊ 0⤋