Find Empirical Formula for Gas X: C_7H_16

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The discussion focuses on determining the empirical formula of a gas, referred to as Gas X, which has a density of 1.187 g/dm³ at 1.01 atm and 35°C, with a composition of 79.8% carbon and 20.2% hydrogen by mass. The initial calculation of the mole ratio of carbon to hydrogen resulted in C₇H₂₀, but it was noted that this formula does not correspond to a known gas. Upon reevaluation, it was recognized that the empirical formula should be simplified to CH₃. The conversation emphasizes the importance of correctly interpreting the empirical formula versus the molecular formula and highlights the need to simplify ratios appropriately, especially when considering the logical constraints of carbon-containing gases.
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A gas X has a density of 1.187gdm^-3 at 1.01 atm. & 35^oC. Gas X contains 79.8% by mass of C & 20.2% by mass of H. Find the empirical formula of X.

Here are my steps:

mole ratio of C to H = 79.8/12.01 : 20.2/1.008
= 7: 20
In that case, its empirical formula is C_{7}H_{20} while I don't think there is a gas with this formula, the closest one is C_{7}H_{16}. Can anyone help me with it?

I know what's wrong now...I have mistaken it as the molecular formula...hheee...being silly...so the answer should be CH_{3}.
 
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Ok.

Note: to make your Latex fit into the text, use "itex" and "/itex" in the brackets instead of "tex" and "/tex".
 
It is very simple; just simplify the ratio, \frac {7}{20} to obtain \frac {1}{0,35}. As you know that a carbon-containing gas must contain up to five carbon atoms, a gas with seven carbons would not be logical. So just simplify the ratio for your needs.
 

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