2Fes - 3-2 O2g - Fe2O3s H - -193-4 kJ - - - - - - 1Mgs - 1-2 O2g - MgOs H - -140-2 kJ - - - - - - 2What is -H of the reaction- 3Mg - Fe2O3 - 3MgO - 2Fe

Equation (2) is multiplied by 3 2Fe(s) + 3/2 O_2(g) → Fe_2O_3(s) H = 193.4 kJ. . . . . . (1) 3Mg(s) + 3/2 O_2(g) → 3MgO(s) H = 420.6 kJ ...

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Hess' Law

2Fes + 3/2 O2...

Question

$2 F e (s) + \frac{3}{2} O_{2} (g) \to F e_{2} O_{3} (s) (△ H = - 193.4 k J) . . . . . . (1)$
$M g (s) + \frac{1}{2} O_{2} (g) \to M g O (s) (△ H = - 140.2 k J) . . . . . . (2)$

What is $△$ ∆H of the reaction? $3 M g + F e_{2} O_{3} \to 3 M g O + 2 F e$

-272.3 kJ

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272.3 kJ

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272.2 kJ

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-227.2 kJ

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Solution

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2 F e (s) + \frac{3}{2} O_{2} (g) \to F e_{2} O_{3} (s) (△ H = - 193.4 k J) . . . . . . (1)

M g (s) + \frac{1}{2} O_{2} (g) \to M g O (s) (△ H = - 140.2 k J) . . . . . . (2)

△

3 M g + F e_{2} O_{3} \to 3 M g O + 2 F e

2 F e (s) + \frac{3}{2} O_{2} (g) ⟶ {F e}_{2} O_{3} (s); Δ H = - 193.4 k J . . . (i)

M g (s) + \frac{1}{2} O_{2} (g) ⟶ M g O (s); Δ H = - 140.2 k J . . . . (i i)

Δ H

3 M g + {F e}_{2} O_{3} ⟶ 3 M g O + 2 F e

F e O (s) + F e_{2} O_{3} (s) \to F e_{3} O_{4} (s)

2 F e (s) + O_{2} (g) \to 2 F e O (s); Δ H^{\circ} = - 544 k J 4 F e (s) + 3 O_{2} (g) \to 2 F e_{2} O_{3} (s); Δ H^{\circ} = - 1648.4 k J F e_{3} O_{4} (s) \to 3 F e (s) + 2 O_{2} (g); Δ H^{\circ} = + 1118.4 k J

F e_{2} O_{3} (s) + 3 H_{2} (g) \to 2 F e (s) + 3 H_{2} O (l)

F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)

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