The following two reactions are knownFe2O3s-3COg- 2Fes-3CO2g- H-26-8 kJFeOs-COg- Fes-CO2g- H-16-5 kJThe value of - H for the following reactionFe2O3s-COg- 2FeOs-CO2g is

As Given in above, Fe_2O_3(s)+3CO(g)→ 2Fe(s)+3CO_2(g); Δ H= 26.8 kJ ...(i) FeO(s)+CO(g)→ Fe(s)+CO_2(s);Δ H= 16.5 kJ ...(ii) Fe_2O_3(s)+CO(g)→ 2FeO(s)+ ...

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Standard XII

Chemistry

Contact Process

The following...

Question

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

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

+10.3 kJ

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-43.3 kJ

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-10.3 kJ

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+6.2 kJ

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Solution

The correct option is D +6.2 kJ
As Given in above, $F e_{2} O_{3 (s)} + 3 C O_{(g)} \to 2 F e_{(s)} + 3 C O_{2 (g)}; Δ H = - 26.8 k J$ ...(i)

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

$F e_{2} O_{3 (s)} + C O_{(g)} \to 2 F e O_{(s)} + C O_{2 (g)}; Δ H = ?$ ...(iii)

Eq. (iii) can be obtained as:

(i) -(ii) = -26.8 - 2(-16.5) = -26.8 + 33.0 = +6.2 kJ
$∴$ the correct option is (d).

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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. Given the following thermos chemical reactions:

X O_{2} (s) + C O (g) \to X O (s) + C O_{2} (g)

;

Δ H = - 20.0

X_{3} O_{4} (s) + C O (g) \to 3 X O (s) + C O_{2} (g)

;

Δ H = + 6.0

3 X_{2} O_{3} (s) + C O (g) \to 2 X_{3} O_{4} (s) + C O_{2} (g)

;

Δ H = - 12.0

Find

Δ H

in kJ for the reaction.

2 X O_{2} (s) + C O (g) \to X_{2} O_{3} (s) + C O_{2} (g)

Q. Calculate

Δ H

k J

for the following reaction:

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

Given that,

H_{2} O (g) + C (g) \to C O (g) + H_{2} (g)

;

Δ H = + 131 k J

C O (g) + \frac{1}{2} O_{2} (g) \to {C O}_{2} (g)

;

Δ H = - 282 k J

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

;

Δ H = - 242 k J

Q. In the reaction,

C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (g); Δ H = 2.8 k J, Δ H

represents :

Q. The heat of formation of

C O (g)

and

C O_{2} (g)

are

Δ H = - 110

and

Δ H = - 393 k J m m o l^{- 1}

respectively. What is the heat of reaction

(Δ H)

(in kJ

m o l^{- 1}

) for the following reaction?

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

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The following two reactions are known Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g);ΔH=−26.8 kJ FeO(s)+CO(g)→Fe(s)+CO2(g);ΔH=−16.5 kJ The value of ΔH for the following reaction Fe2O3(s)+CO(g)→2FeO(s)+CO2(g) is