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Stoichiometric Calculations

Three samples...

Question

Three samples of iron equal weights are used to from FeO, ${F e}_{2} O_{3}$ and ${F e}_{3} O_{4}$ independently. Then, the amount (in grams)
of $O_{2}$ required is

A

maximum for the formation of

{F e}_{3} O_{4}

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B

maximum for the formation of

{F e}_{2} O_{3}

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C

minimum for the formation of

{F e}_{2} O_{3}

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D

the same for the formation of all the three

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Solution

The correct option is A maximum for the formation of ${F e}_{2} O_{3}$
Mole ratio of oxygen that combines with mole of Fe
$F e O = 1 = 1$
${F e}_{\frac{3}{2}} = \frac{3}{2} =$ 1.5
${F e}_{3} O_{4} = \frac{4}{3} =$ 1.33

So, max. is for ${F e}_{2} O_{3}$

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Similar questions

Δ G = - 177 K c a l

(1) 2 F e (s) + \frac{3}{2} O_{2} (g) ⟶ {F e}_{2} O_{3} (s)

Δ G = - 19 K c a l f o r (2) {4 F e}_{2} O_{3} (s) ⟶ {3 F e}_{3} O_{4} (s)

What is the Gibbs free energy of formation of

{F e}_{3} O_{4}

?

Q. Mole ratio of

F e

F e O

{F e}_{2} O_{3}

{F e}_{3} O_{4}

samples of equal mass is:

Q. The standard enthalpy of formation of

H_{2} O (l)

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

are respectively

- 286

k J

{m o l}^{- 1}

- 824

k J

{m o l}^{- 1}

. What is the standard enthalpy change for the following reaction?

{F e}_{2} O_{3} (s) + 3 H_{2} (g) ⟶ 3 H_{2} O (l) + 2 F e (s)

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. 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

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