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An ideal gas is $\text{84% carbon}$ and $\text{16% hydrogen}$ by weight.

If the gas has a density of $4.67\text{ g/L}$ at a temperature of ${25}^{o}C$ and a pressure of $1.00\text{ atm}$, what is the molecular formula of the gas?

$\left(R=0.0821\frac{L\times atm}{mol\times K}\right)$

A

${C}_{5}{H}_{12}(g)$

B

${C}_{6}{H}_{14}(g)$

C

${C}_{7}{H}_{16}(g)$

D

${C}_{8}{H}_{18}(g)$

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