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[tex]\Delta H^{\circ}_{diss}[/tex] (O-O) = 251 kJ

[tex]\Delta H^{\circ}_{diss}[/tex] (O-H) = 465 kJ

[tex]\Delta H^{\circ}_{diss}[/tex] (H-H) = 435 kJ

[tex]\Delta H^{\circ}_{diss}[/tex] (Na-O) = 255 kJ

[tex]\Delta H_{sol}[/tex] = -46 KJ for [tex]NaOH_{(s)}[/tex]

[tex]NaOH_{(s)} \rightarrow Na^{+}_{(aq)} + OH^{-}_{(aq)} \cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot[/tex][tex]\Delta H[/tex] = -46 KJ

[tex]\Delta H^{\circ}_{f}[/tex] = -427 KJ for [tex]NaOH_{(s)}[/tex]

[tex]Na_{(s)} + \frac{1}{2}O_{2(g)} + \frac{1}{2}H_{2(g)} \rightarrow NaOH_{(s)} \cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot\cdot[/tex][tex]\Delta H[/tex] = -427 KJ

I forgot one part:

[tex]Na_{(s)} \rightarrow Na_{(g)} \cdot\cdot\cdot\cdot\cdot \Delta H[/tex] = 109 kJ

Predict [tex]\Delta H[/tex] for [tex]NaOH_{(s)} \rightarrow NaOH_{(g)}[/tex]

Because im trying to find the enthalpy of one reaction, and i have other 'known' enthalpy reactions does this problem automatically turn into a Hess' Law type problem ? or is this still a bond energy/enthalpy reaction or just bond energy type problem ? Also i do not have a [tex]NaOH_{(g)}[/tex] in any of my reaction so how can i go about computing the targeted enthalpy ?

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# Homework Help: NaOH(s) -> NaOH(g)

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