chemical equation; determination of organic compound?

Question

A certain compound was found to have a molar mass of 60.095 g. A 3.470 g sample of this compound was burned in pure oxygen gas. The measured amount of CO2 produced was 7.623 g, while that of H2O was 4.161 g. No other products were produced in the reaction.

How many moles of hydrogen were in the original sample that underwent combustion ?

Answer 1

Most of the info provided is superfluous.
Simply put, you burned something and got 4.161g H2O (MW=18.016), all H coming from the sample.
So you formed 4.161/18.016 = 0.23096 mols H2O, and since each mol H2O contains 2 mols H, your sample contained 0.4619 mols of H.

BTW, it is easy to deduce the empirical formula of the compound:
No hydrocarbon can have a MW of 60.095, and since only CO2 and H2O were formed, the compound must contain O...this works out to be C3H8O, which means it is probably propanol (n or iso) or methyl ethyl ether.

Answer 2

that's balanced, because of the fact you have the comparable variety of each and every ingredient on the two sides of the equation! KOH+H2SO4 -> KHSO4+H2O that's composed of all organic and organic compounds because of the fact they're all usually happening metals and that's what organic and organic chemistry is. it relatively relies on the ingredient Carbon C6H6, C2H5OH, C6H5CH3, C3H5(NO3)3 that's the main appropriate thank you to stability the equation because of the fact it has the comparable variety or each and every ingredient on the two sides. CO2 + C ? 2CO i'm hoping this helped, in case you have any greater suitable questions i'd be satisfied to help!

Answer 3

moles compound x: 3.470g / 60.095g/mol = 0.05774 mol
moles CO2: 7.623g / 44g/mol = 0.1732 mol
moles H2O: 4.161g / 18g/mol = 0.2312 mol

balance equation:
compound x + 5O2 ---> 3CO2 + 4H2O

Number of moles of H that underwent combustion:
8 * 0.05774 mol = 0.4619 mol

Answer: 0.4619 moles of H

Answer 4

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