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Heat of Formation

From the data...

Question

From the data at $25^{o} C$ :
${F e}_{2} O_{3} (s) + 3 C_{g r a p h i t e} ⟶ 2 F e (s) + 3 C O (g); Δ H^{o} = 492 k J / m o l$
$F e O (s) + C_{g r a p h i t e} ⟶ F e (s) + C O (g); Δ H^{o} = 155.8 k J / m o l$
$C_{g r a p h i t e} + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 393.51 k J / m o l$
$C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 282.98 k J / m o l$
Calculate standard heats of formation of $F e O (s)$ and ${F e}_{2} O_{3} (s)$ .

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Solution

$F e O (s) + C_{g r a p h i t e} ⟶ F e (s) + C O (g); Δ H^{o} = 155.8 k J / m o l$
$C_{g r a p h i t e} + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 393.51 k J / m o l$
$C O_{2} (g) ⟶ C O (g) + \frac{1}{2} O_{2} (g); Δ H^{o} = - 282.98 k J / m o l$
On adding
$F e (s) + \frac{1}{2} O_{2} (g) ⟶ F e O (s); Δ H = - 266.3 k J / m o l$
Similarly we may calculate heat of formation of ${F e}_{2} O_{3}$

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Similar questions

Q. From the following data at 25C, Calculate the standard enthalpy of formation of FeO(s) and of

{F e}_{2} O_{3} (s)

.

	Reaction	$Δ_{r} H (K J / m o l e)$
(1)	${F e}_{2} O_{3} (s) + 3 C (g r a p h i t e) \to 2 F e (s) + C O (g)$	492
(2)	$F e O (s) + C (g r a p h i t e) \to F e (s) + C O (g)$	155
(3)	$C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g)$	-393
(4)	$C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g)$	-282

Q. From the following data at

25^{\circ} C

, The standard enthalpy of formation of FeO(s) is X, then 0.3-X is:

Reaction	$Δ_{r} H^{\circ}$ ( kJ / mole )
$F e_{2} O_{3} (s) + 3 C (g r a p h i t e) \to 2 F e (s) + 3 C O (g)$	492.6
$F e O (s) + C (g r a p h i t e) \to F e (s) + C O (g)$	155.8
$C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g)$	$-$ 393.51
$C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g)$	$-$ 282.98

Q. Calculate the standard enthalpy of formation of

C H_{3} O H (l)

from the following data.

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

Δ H^{o} = - 726

m o l^{- 1}

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

Δ_{c} H^{0} = - 393

m o l^{- 1}

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

Δ_{t} H^{o} = - 286

m o l^{- 1}

.

Q. Determine the heat of the following reaction:

F e O (s) + {F e}_{2} O_{3} (s) ⟶ {F e}_{3} O_{4} (s)

Given informations:

2 F e (s) + O_{2} (g) ⟶ 2 F e O (s); Δ H^{o} = - 544 k J

4 F e (s) + 3 O_{2} (g) ⟶ 2 {F e}_{2} O_{; 3} (s); Δ H^{o} = - 1648.4 k J

{F e}_{3} O_{4} (s) ⟶ 3 F e (s) + 2 O_{2} (g); Δ H^{o} = + 1118.4 k J

Q. Calculate the

Δ H

C (g r a p h i t e) \to C (d i a m o n d)

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

C (g r a p h i t e) + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 395.4 k J

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