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.

Question

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. (A) 95.3 kJ (B) 8900 kJ (C) 890 kJ (D) 8.9 kJ

Tardigrade Admin · Accepted Answer

CH 4( g )+2 O 2( g ) longrightarrow CO 2( g )+2 H 2 O (l) ; Δ H Δ H is 890 kJ for 1 mole CH 4 We know, 22.4 L means 1 mol 2.4 L means (1/22.4) × 2.4 mol =0.107 mol ∴ Δ H=890 kJ × 0.107=95.23 kJ

Q. The heat liberated on complete combustion of 1 mole of $C H_{4}$ gas to $C O_{2} (g)$ and $H_{2} O (l)$ is $890 k J$ . Calculate the heat evolved by $2.4 L$ of $C H_{4}$ on complete combustion.

95.3 kJ

8900 kJ

890 kJ

8.9 kJ

$C H_{4} (g) + 2 O_{2} (g) ⟶ C O_{2} (g) + 2 H_{2} O (l); Δ H$
$Δ H$ is $890 k J$ for $1$ mole $C H_{4}$
We know, $22.4 L$ means $1$ mol
$2.4 L$ means $\frac{1}{22.4} \times 2.4 m o l = 0.107 m o l$
$∴ Δ H = 890 k J \times 0.107 = 95.23 k J$

Q. The heat liberated on complete combustion of 1 mole of CH4​ gas to CO2​(g) and H2​O(l) is 890kJ. Calculate the heat evolved by 2.4L of CH4​ on complete combustion.