Question

The heat liberated on complete combustion of
1 mole of CH4 gas to CO2(g) and H2O(1) is 890 kJ.
Calculate the heat evolved by 2.4 L of CH, on
complete combustion.
(1) 95.3 kJ
(2) 8900 kJ
(3) 890 kJ
(4) 8.9 kJ​

Answer 1

The heat evolved by 2.4 L of $CH_4$ on  complete combustion is 95.3 kJ

complete combustion.

Explanation:

Heat of combustion is the amount of heat released on complete combustion of 1 mole of substance.

$CH_4+2O_2\rightarrow CO_2+2H_2O$

Given :

Amount of heat released on combustion of 1 mole of methane= 890 kJ/mol

According to avogadro's law, 1 mole of every substance occupies 22.4 L at NTP, weighs equal to the molecular mass and contains avogadro's number $6.023\times 10^{23}$ of particles.

Moles of methane =$\frac{\text{ given volume}}{\text{ molar volume}}= \frac{2.4L}{22.4L/mol}=0.107moles$

Thus we can say:  

1 mole of $CH_{4}$ on combustion releases =890 kJ

Thus 0.11 moles of $CH_{4}$ on combustion releases =$\frac{890}{1}\times 0.11=95.3kJ$

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