The enthalpy of reaction for the reaction-2H2g - O2 g - 2H2Ol is -rHo - -572 kJ mol-1What will be standard enthalpy of formation of H2Ol-

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Natural and Man-made Chemical Changes

The enthalpy ...

Question

The enthalpy of reaction for the reaction:

$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ is
$Δ_{r} H^{o} = - 572 k J m o l^{- 1}$

What will be standard enthalpy of formation of $H_{2} O (l)$ ?

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2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l) i s Δ_{r} H^{o} = - 572 k J m o l^{- 1}

H_{2} O (l)

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

N_{2} H_{4} (l) + 2 H_{2} O_{2} (l) \to N_{2} (g) + 4 H_{2} O (l);

△_{r} H_{1}^{o} = - 818 k J / m o l

N_{2} H_{4} (l) + O_{2} (g) \to N_{2} (g) + 2 H_{2} O (l);

△_{r} H_{2}^{o} = - 622 k J / m o l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); △_{f} H_{3}^{o} = - 285 k J / m o l

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

H_{2} O_{2} (l)

H_{2} O (l)

- 188

- 286 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l) i s Δ_{r} H^{o} = - 572 k J m o l^{- 1}

H_{2} O (l)

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)

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