Question

A 5.347 g of hexane undergo combustion.

g H₂O generated?

Answer 1

The balanced chemical equation for the combustion of hexane is:

$2C_6H_{14}+19O_2 \to 12CO_2+14H_2O$

RMM for hexane = $6\times 12+1\times 14=86$

Moles of hexane used $=0.0623moles$

mole ratio $C_6H_{14}:CO_2=2:12$

Moles of $CO_2=12/2\times 0.0623=0.3738moles$

Mass of $CO_2=0.3738 \times (12+16+16)=16.4472g$

mole ratio $C_6H_{14}:H_2O=2:14$

Moles of $H_2O =14/2\times 0.0623=0.4361moles$

mass of $H_2O$ produced = $0.4361\times (1+1+16)=7.8498$