Calculate - H for the reaction between ethene and water to form ethyl alcohol from the following data- -cHC2H5OHI - -1368 kJ -cHC2H4g - -1410 kJDoes the calculated - H0 represent the enthalpy of formation of liquid ethanol-

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Heat of Formation

Calculate Δ...

Question

Calculate $Δ H$ for the reaction between ethene and water to form ethyl alcohol from the following data:
$Δ_{c} H C_{2} H_{5} {O H}_{(I)} = - 1368 k J$
$Δ_{c} H C_{2} H_{4 (g)} = - 1410 k J$
Does the calculated ${Δ H}^{0}$ represent the enthalpy of formation of liquid ethanol?

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Δ H^{o}

Δ_{c} H^{o} C_{2} H_{5} O H_{(l)} = - 1368 k J

Δ_{c} H^{o} C_{2} H_{4 (g)} = - 1410 k J

Δ H^{o}

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ_{r} H^{\circ} = - 1368.0 k J

C (s) + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)

Δ_{r} H^{\circ} = - 286.0 k J

Δ H

H_{2} (g) + B r_{2} (l) ⟶ 2 H B r (g)

C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 286.2 k J

C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 1410.8 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = - 94 K c a l

H_{2} (g) + I / 2 O_{2} (g) ⟶ H_{2} O (l)

Δ H = - 68 K c a l

C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 327 K c a l

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