For the reaction, 2H2(g) +O2 (g) → 2H2O(g) , Δ H° = -573.2 kJ The heat of decomposition of water per mole is

Question

For the reaction, 2H2(g) +O2 (g) → 2H2O(g) , Δ H° = -573.2 kJ The heat of decomposition of water per mole is (A)  286.6 kJ  (B)  573.2 kJ  (C)  -28.66 kJ  (D) zero

Tardigrade Admin · Accepted Answer

Heat of decomposition of water is H 2 O (g) longrightarrow H 2(g)+(1/2) O 2(g) Δ H =(+573.2/2) = 286.6 kJ / mol

Q. For the reaction,
$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (g)$ , $Δ H^{\circ} = - 573.2 k J$
The heat of decomposition of water per mole is

$286.6 k J$

$573.2 k J$

$- 28.66 k J$

zero

Heat of decomposition of water is

$H_{2} O (g) ⟶ H_{2} (g) + \frac{1}{2} O_{2} (g)$

$Δ H = \frac{+ 573.2}{2}$

$= 286.6 k J / m o l$

Q. For the reaction, 2H2​(g)+O2​(g)→2H2​O(g) , ΔH∘=−573.2kJ The heat of decomposition of water per mole is

286.6kJ

573.2kJ

−28.66kJ