Find the value of - H- for the reaction- Fe2O3s - 3CO2g - 2Fes - 3CO2g-

The given reaction is: Fe_2O_3(s)+3CO(g)→ 2Fe(s)+3CO_2(g) The value of Δ H^∘_f,Fe_2O_3(s)= 825.50 kJ/mol The value of Δ H^∘_f,CO(g)= 110.53 kJ/mol ...

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Standard XII

Chemistry

Relation between Cp and Cv

Find the valu...

Question

Find the value of $Δ H^{\circ}$ for the reaction, $F e_{2} O_{3} (s) + 3 C O_{2} (g) \to 2 F e (s) + 3 C O_{2} (g)$ .

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Solution

The given reaction is:
$F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g)$

The value of $Δ H_{f, F e_{2} O_{3} (s)}^{\circ} = - 825.50 k J / m o l$
The value of $Δ H_{f, C O (g)}^{\circ} = - 110.53 k J / m o l$
The value of $Δ H_{f, C O_{2} (g)}^{\circ} = - 393.52 k J / m o l$

The enthalpy of a reaction is given by
$Δ H^{\circ} = \sum_{v_{p}} Δ H_{f, p}^{\circ} - \sum_{v_{r}} Δ H_{f, p}^{\circ}$
where, $v_{p}$ is the stoichiometric coefficient of the product an the reactant;
$Δ H_{f}^{\circ}$ is the standard enthalpy of formation of a substance.

Putting the values of $Δ H_{f}^{\circ}$ for each compound in the given reaction, we can calculate the enthalpy of formation for the reaction as follows :
$Δ H^{\circ} = [2 \times 0 + 3 \times (- 393.52)] - [1 \times (- 825.50) + 3 \times (- 110.53)]$
$\Rightarrow Δ H^{\circ} = (0 - 1180.56 + 825.50 + 331.59) k J / m o l$
$\Rightarrow Δ H^{\circ} = - 23.47 k J / m o l$

Therefore, the value of $Δ H^{\circ}$ for the given reaction is $- 23.47 k J / m o l$ .

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Similar questions

Q. The following two reactions are known

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

;

Δ H = - 26.8 k J

F e O_{(s)} + C O_{(g)} \to F e_{(s)} + C O_{2 (g)} Δ H = - 16.5 k J

The value of

Δ H

for the following reaction is:

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

Q. Justify that the following reactions are redox reactions:

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

Q. The following two reactions are known

F e_{2} O_{3 (s)} + 3 C O_{(g)} \to 2 F e_{(s)} + 3 C O_{2 (g)}; Δ H = - 26.8 k J

F e O_{(s)} + C O_{(g)} \to F e_{(s)} + C O_{2 (g)}; Δ H = - 16.5 k J

The value of

Δ H

for the following reaction

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

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. For the reaction,

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

which of the following is correct?

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Find the value of ΔH∘ for the reaction, Fe2O3(s)+3CO2(g)→2Fe(s)+3CO2(g).

Find the value of $Δ H^{\circ}$ for the reaction, $F e_{2} O_{3} (s) + 3 C O_{2} (g) \to 2 F e (s) + 3 C O_{2} (g)$ .