Find the heat of formation of ethyl alcohol from following data Cs - O2g- CO2g- - H - -94 Kcal H2g - I-2O2g- H2Ol- - H - -68 Kcal C2H5OHl - 3O2g- 2CO2g - 3H2Ol- - H - -327 Kcal

The correct option is A 65 Kcal mol^ 1 2C(s) + 3H_2(g)+ 1 / 2 O_2(s)⟶ C_2H_5OH(l) #160;Given: C(s) + O_2(g)⟶Δ H_1 = 94 Kcal CO_2(g) .....(i ...

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Le Chatelier's Principle for Del N Equals to 0

Find the heat...

Question

Find the heat of formation of ethyl alcohol from following data
$C (s) + O_{2} (g) ⟶ C O_{2} (g)$ ...... $Δ H = - 94 K c a l$
$H_{2} (g) + I / 2 O_{2} (g) ⟶ H_{2} O (l)$ ;.... $Δ H = - 68 K c a l$
$C_{2} H_{5} O H (l) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l)$ ..... $Δ H = - 327 K c a l$

65 K c a l m o l^{- 1}

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85 K c a l m o l^{- 1}

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- 65 K c a l m o l^{- 1}

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None of these

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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

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 394 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l); Δ H = - 568 k J / m o l

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l); Δ H = - 1058 k J / m o l

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

Δ H = - 94.0 K c a l

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

Δ H = - 68.0 K c a l

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

Δ H = - 210.0 K c a l

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = - 393.7 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l)

Δ H = - 285.8 k J

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

Δ H = - 873.2 k J

{C H}_{3} O H (l)

{C H}_{3} O H (l) + \frac{3}{2} O_{2} (g) ⟶ C O_{2} (g) + 2 H_{2} O (l); Δ H = - 726 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 394 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 286 k J

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