Question #7925

The analysis of a hydrocarbon revealed that it was 85.6281% C and 14.3719% H by mass. When 2.94 g of the gas was stored in a 1.4 L flask at −32.1762C, it exerted a pressure of 450 Torr. What is the molecular formula of the hydrocarbon?

Expert's answer

Mol C = 85.6281 g / 12.011 = 7.1291

Moles H = 14.3719 g / 1.00794 = 14.259

we divide by the smallest number empirical formula CH_{2} (mass = 14.0269 g/mol)

p = 450/760 = 0.592 atm

T = −32.1762 + 273 = 240.8238 K

moles = pV / RT = 0.592 *1.4/ 0.0831* 240,8238 = 0.0414

Molar mass = 2.94 g / 0.0414 = 71.014 g/mol

71.014 / 14.0269 = 5

we multiply the empirical formula by 5 and we get C_{5}H_{10}

Moles H = 14.3719 g / 1.00794 = 14.259

we divide by the smallest number empirical formula CH

p = 450/760 = 0.592 atm

T = −32.1762 + 273 = 240.8238 K

moles = pV / RT = 0.592 *1.4/ 0.0831* 240,8238 = 0.0414

Molar mass = 2.94 g / 0.0414 = 71.014 g/mol

71.014 / 14.0269 = 5

we multiply the empirical formula by 5 and we get C

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