Gas is either CH4 or C2H6. A 1.00-g sample of this gas produces 1.80 g of water ...

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September 2022 1 1 Report

Gas is either CH4 or C2H6. A 1.00-g sample of this gas produces 1.80 g of water when combusted in excess O2. Assuming complete combustion to CO2 and H2O, which gas is it?

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indrawboy

Verified answer

Reaction

$\tt C_xH_y+O_2\Rightarrow CO_2+H_2O$

mass H before reaction = mass H after reaction ⇒ complete combustion

Mass H in H₂O : mass H in gas

$\tt =\dfrac{2.Ar~H}{MW~H_2O}\times mass~H_2O\\\\=\dfrac{2\times 1.0079}{18.0152}\times 1.8~gr\\\\=0.20141~gr$

Mass C in sample :

$\tt 1~gr-0.20141=0.79859~gr$

Empirical Formula = mol ratio of the compound

mol ratio = C : H ⇒

$\tt =\dfrac{0.79859}{12}:\dfrac{0.20141}{1.0079}\\\\=0.06655\div 0.19983\\\\=1\div 3$

So the Empirical Formula of the gas : CH₃ or the molecular formula : C₂H₆

GwaposiMark what is the unit gr?

GwaposiMark Can you explain again the process and where did you get the units that you have used SIr?

indrawboy gr=grams

GwaposiMark What is the unit Ar mean the same as to MW?

indrawboy Ar=relative atomic mass(for atom) , MW=molecular weight(for molecul/compound)

indrawboy you can use another way to find the gas by mol ratio between 2 combustion reaction (CH4 and C2H6)

GwaposiMark how Sir?

indrawboy hehe..you can find it okey..keep learning..thank you..

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