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Ede4ka [16]
3 years ago
14

A gaseous hydrogen and carbon containing compound is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass.

The mass of 158 mL of the gas, measured at 556 mmHg and 25 ∘C, was found to be 0.275 g. What is the molecular formula of the compound?
Chemistry
1 answer:
Doss [256]3 years ago
3 0
For the answer to the question above, I'll show the solution to my answers

moles C = 82.66 g/ 12.0111 g/mol=6.882 
<span>moles H = 17.34 g/ 1.008 g/mol=17.20 </span>

<span>17.20/ 6.882 =2.5 => H </span>
<span>6.882 / 6.882 = 1 => C </span>

<span>to get whole numbers multiply by 2 </span>
<span>C2H5 ( empirical formula Molar mass = 29.062 g/mol) </span>

<span>n = pV/RT = 0.732 x 0.158 L/ 0.08206 x 298 K= 0.00473 </span>
<span>molar mass = 0.275/ 0.00473 =58.1 g/mol </span>

<span>58.1 / 29.062 = 2 </span>

<span>multiply by two the empirical formula </span>

<span>C4H10</span>
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