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Calorimetry

If Δ Hof fo...

Question

If $Δ H_{f}^{o}$ for $H_{2} O_{2}$ and $H_{2} O$ are -188kJ / mole and -286 kJ / mole. What will be the enthalpy change of the reaction $2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)$ ?

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Solution

$Δ H_{r x n} = \sum Δ H_{p r o d u c t} - \sum Δ H_{p r o d u c t}$
$2 H_{2} O_{2} (l) ⟶ 2 H_{2} O (l) + O_{2} (g)$
$Δ H_{r x n} = (2 \times - 286) - (2 \times - 188) = - 572 + 376 = - 196$ $k J / m o l$

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Similar questions

Δ H_{f}^{0}

H_{2} O_{2}

H_{2} O

2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)

Δ H_{f}^{o}

H_{2} O_{2} (l)

H_{2} O (l)

- 188 k J

{m o l}^{- 1}

- 286 k J

{m o l}^{- 1}

2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)

2 H_{2} O_{2} (l)

\to

2 H_{2} O (l)

H_{2} O

H_{2} O_{2}

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

H_{2} O

- 188

H_{2} O_{2}

- 286

2 H_{2} O_{2} \to 2 H_{2} O + O_{2}

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