Question help

[EmmaQuinn]

Am struggling with this question - An unknown organic compound was analysed to determine identity. It contained, C, H and O, it had no carbon-carbon double bonds. When completely oxidised in air, 8.20 g of the compound produced 8.19g of water and 20.2g of carbon dioxide.

I. based on the mass of water produced by the oxidation, calculate the mass of hydrogen in the 8.20g sample of the compound??


Thanks

[Swagadaktal]

aight so assume its a complete oxidation reaction.

You have:
n(H2O) = 8.19/18 = 0.455 mol, n(CO2) = 20.2/44 = 0.459 mol CO2
The reaction goes as follows.
(Unknown hoe) +  (x)O2 --> 0.455H2O + 0.459CO2 (cbf with states true?)
we can deduce the amount of oxygen. We have 0.459 mol of CO2 which equals 0.459 mol O2, and we have that 0.455mol of O from H2O so that's 0.2275 mol O2. Adding them up we get 0.687 mol O2 in the whole thing.

Now we gotta see how many carbons we got. We have 0.459 mol CO2 soo 0.459 mol C. ez.
Now we can't forget about our OG Hoe: Hydrogen. 0.455 mol of H2 means 0.91 mol of H. Now, coz we know that it's a saturated organic compound, it only has 2 oxygens per molecule yeah? (The COOH group at the end.)

OK SO FK ME I DIDNT READ THE QUESTION YOU JUST WANNA WORK OUT THE MASS OF HYDROGEN I WAS TRYNA WORK OUT MASS OF CARBON

Mass of hydrogen: U produce 0.455 mol of H2O meaning 0.91 mol H2 which is 1.82g - This is all you need lmfao

Btw anyone reading this - I think i made a mistake somewhere earlier and am I correct with this last statement?

[EmmaQuinn]

Okay so I understand that the mol of H20 is 0.455, but how did you get the 0.91 mol of H2 in the 8.2g organic compound..?
Sorry don't know why I cn't get my head around it :O

[Swagadaktal]

Okay so I understand that the mol of H20 is 0.455, but how did you get the 0.91 mol of H2 in the 8.2g organic compound..?
Sorry don't know why I cn't get my head around it :O

Ooh soz i derped it out i meant 0.91 mol of H which is 0.91g sozz mb