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Stoicheometry?
I have no clue how to solve these problems. Would you please help me figure out. Thank you.
A 0.2417g sample of a compound composed of C,H,O,Cl only, is burned in oxygwn yielding 0.4964g of CO2 and 0.0846g of H2O. A separate 0.1696g sample of the compound is fused with sodium metal, the products dissolved in water and the chloride quantitatively precipitated with AgNO3 to yield 0.1891g of AgCl. What is the simplest empirical formula for the compound.
A 14.1 mg sample of a hydrocarbon was burned in air. The products were 38.8 mg of CO2 and 31.7 mg of water. what is the emppirical formula of the hydrocarbon.
1 Answer
- 1 decade agoFavorite Answer
find the moles of each C from CO2 H from H2O (remember to times by 2) use the mass of AgCl to find moles of Cl (you need to set up a proportion from one sample to the next). conver all of those moles to masses...add them up and subtract the mass of CHand Cl from the total to find the mass of the missing O. convert the mass of O to moles. find the mole ratio of the 4 and that is the empirical formula.
The second is much easier just find the mole ratio of carbon using CO2 and H using H2O and times that by 2
I used your questions as an example on my website.
