For the following equation, ${F e}_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 {C O}_{2} (g)$ , when 3.0 mol ${F e}_{2} O_{3}$ is allowed to completely react with 56 g $C O$ , approximately how many moles of iron, $F e$ , are produced?

0.7

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1.3

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2.0

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2.7

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6.0

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Solution

The correct option is A $1.3$
The atomic masses of $C$ and $O$ are 12 g/mol and 16 g/mol respectively.
The molar mass of $C O$ is $12 + 16 = 28$ g/mol.
56 g $C O$ corresponds to $\frac{56}{28} = 2$ moles.
As per balanced chemical equation, 1 mole of $F e_{2} O_{3}$ will react with 3 moles of $C O$ .
Hence, 3.0 moles of $F e_{2} O_{3}$ will react with $3.0 \times 3 = 9$ moles of $C O$ .
However only 2 moles of $C O$ are present. Hence, $C O$ is the limiting reagent and $F e_{2} O_{3}$ is excess reagent.
As per the balanced chemical equation, 3 moles of $C O$ produces 2 moles of $F e$ .
Hence, 2 moles of $C O$ will produce $2 \times \frac{2}{3} = 1.3$ moles of $F e$ .

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2 H_{2} S (g) + 3 O_{2} (g) \to 2 S O_{2} (g) + 2 H_{2} O (g) +

heat

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

According to the above reaction , 3 moles of $F e_{2} O_{3}$ are allowed react with 56 grams of CO so, find the approximately moles of iron produced ?

Q. Calculate, the

Δ H

85^{o} C

for the reaction:

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

The data are:

Δ H_{298}^{o} = - 33.29 k J / m o l

and

Substance	${F e}_{2} O_{3} (s)$	$F e (s)$	$H_{2} O (l)$	$H_{2} (g)$
$C_{P}^{o} (J / K m o l)$	$103.8$	$25.1$	$75.3$	$28.8$

Q. 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)

{F e}_{2} O_{3} + 3 C O \to 2 F e + 3 {C O}_{2} F e O + C O \to F e + {C O}_{2} △ r_{H} = - 26 k J △ r_{H} = - 16 k J

Find

△ H

of reaction

{F e}_{2} O_{3} + C O \to 2 F e O + {C O}_{2} △ r_{H} = ?

2 A l (s) + {F e}_{2} O_{3} (s) ⟶ {A l}_{2} O_{3} (s) + 2 F e (s)

According to the equation for the reaction represented above, which of the following statements is true?

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For the following equation, Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g), when 3.0 mol Fe2O3 is allowed to completely react with 56 g CO, approximately how many moles of iron, Fe, are produced?

For the following equation, ${F e}_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 {C O}_{2} (g)$ , when 3.0 mol ${F e}_{2} O_{3}$ is allowed to completely react with 56 g $C O$ , approximately how many moles of iron, $F e$ , are produced?