Calculate enthalpy for formation of ethylene from the following data-I Cgraphite - O2 g - CO2 g- - H - -393-5 kJII H2g - 12 O2 g - H2Ol- - H - - 286-2 kJIII C2H4g - 3O2g - 2CO2g - 2H2 Ol- - H - - 1410-8 kJ

The correct option is C 51.4 kJ(I) C(graphite) + O_2 (g) → CO_2 (g) #160; #160;— 1(II) H_2(g) + 12 O_2 (g) → H_2O(l) —– 2(III) C_2H_4(g) ...

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Hess' Law

Calculate ent...

Question

Calculate enthalpy for formation of ethylene from the following data:

(I) $C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J$
(II) $H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 286.2 k J$
(III) $C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 1410.8 k J$

54.1 kJ

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44.8 kJ

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51.4 kJ

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48.4 kJ

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Solution

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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

6 C (s) + 3 H_{2} (g) \to C_{6} H_{6} (l); Δ H = + 45.9 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 285.9 k J

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 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

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 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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