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  3. Chemistry
  4. The heat liberated on complete combustion of 1 mole of CH4 gas to CO2(g) and H2O(l) is 890 kJ. Calculate the heat evolved by 2.4 L of CH4 on complete combustion.

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Q. The heat liberated on complete combustion of 1 mole of $CH_4$ gas to $CO_2(g)$ and $H_2O(l)$ is $890 \,kJ$. Calculate the heat evolved by $2.4 \,L$ of $CH_4$ on complete combustion.

Thermodynamics

Solution:

$CH _{4}( g )+2 O _{2}( g ) \longrightarrow CO _{2}( g )+2 H _{2} O (l) ; \Delta H$
$\Delta H$ is $890 \,kJ$ for $1$ mole $CH _{4}$
We know, $22.4\, L\,\,$ means $1$ mol
$2.4\, L \,\,$ means $\frac{1}{22.4} \times 2.4 \,mol =0.107\, mol$
$\therefore \Delta H=890 \,kJ \times 0.107=95.23 \,kJ$