Cs-O2gCO2g- H-393-5 kJ mol-1Cs-12O2gCOg- H-110-5 kJ mol-1H2g-12O2gH2Og- H-241-8 kJ mol-1The standard enthalpy change in kJ mol-1 for the reaction-CO2g - H2 g - COg - H2Og is

Answer (2) CO_2(g) nbsp;→ C(s) + O_2(g) + 393.5 kJ mol^ 1 C(s) + 12O_2(g)→ CO(g) 110.5 kJ mol^ 1 H_2(g) + 12O_2(g)→ H_2O(g) 241.8 kJ mol 1 nbsp; ...

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Byju's Answer

Standard XII

Chemistry

Characteristics of Equilibrium Constant

Cs+O2gCO2gΔ H...

Question

$C (s) + O_{2} (g) - \to C O_{2} (g) Δ H^{\circ} = - 393.5 {kJ mol}^{- 1}$
$C (s) + \frac{1}{2} O_{2} (g) - \to C O (g) Δ H^{\circ} = - 110.5 {kJ mol}^{- 1}$
$H_{2} (g) + \frac{1}{2} O_{2} (g) - \to H_{2} O (g) Δ H^{\circ} = - 241.8 {kJ mol}^{- 1}$
The standard enthalpy change $({in kJ mol}^{- 1})$ for the reaction.
$C O_{2} (g) + H_{2} (g) ⟶ C O (g) + H_{2} O (g)$ is

- 262.2

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+ 41.2

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- 41.2

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+ 262.2

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Solution

The correct option is B $+ 41.2$
Answer (2)
$C O_{2} (g) \to C (s) + O_{2} (g) + 393.5 {kJ mol}^{- 1}$
$C (s) + \frac{1}{2} O_{2} (g) \to C O (g) - 110.5 {kJ mol}^{- 1}$
$H_{2 } (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (g) - 241.8 kJ mol - 1$

Adding: $C O_{2} (g) + H_{2 } (g) \to C O (g) + H_{2} O (g)$

$Δ H_{rnx}^{\circ} = (+ 393.5 - 110.5 - 241.8) {kJmol}^{- 1}$
$= 41.2 {kJmol}^{- 1}$

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Similar questions

Q. The

Δ_{f} H^{o}

for the

C O_{2} (g), C O (g)

and

H_{2} O (l)

are -393.5, -110.5 and -241.8

k J m o l^{- 1}

respectively. The standard enthalpy change (in

k J m o l^{- 1}

) for the given reaction is :

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

Q. The

Δ_{f} H^{0}

for

C O_{2} (g), C O (g) a n d H_{2} O (g)

are -393.5, -110.5 and -241.8

k J m o l^{- 1}

respectively. The standard enthalpy change (in

k J m o l^{- 1}

) for the reaction

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

is :

Q. The

Δ H_{t}^{\circ}

for

C O_{2 (g)}, C O_{(g)}

and

H_{2} O_{(g)}

are

- 393.5, - 110.5

and

- 241.8 k J m o l^{- 1}

respectively the standard enthalpy change (in

K J

) for the reaction

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

is:

Q. The

Δ H_{f}^{o}

for

C O_{2 (g)}

C O_{(g)}

and

H_{2} O_{(g)}

are

- 393.5

- 110.5

and

- 241.8

m o l^{- 1}

respectively the standard enthalpy change (in KJ) for the reaction

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

is:

Q. The

Δ_{f} H^{⊖}

for

C O_{2} (g), C O (g) a n d H_{2} O (g)

are

- 393.5, - 110.5 a n d - 214.8 k J m o l^{- 1}

, respectively. The standard enthalpy change

(i n k J m o l^{- 1})

for the reaction

C O_{2} (g) + H_{2} (g) ⟶ C O (g) + H_{2} O (g)

is:

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C(s)+O2(g)−→ CO2(g)ΔH∘=−393.5 kJ mol−1 C(s)+12O2(g)−→ CO(g)ΔH∘=−110.5 kJ mol−1 H2(g)+12O2(g)−→ H2O(g)ΔH∘=−241.8 kJ mol−1 The standard enthalpy change ( in kJ mol−1) for the reaction. CO2(g)+H2(g)⟶CO(g)+H2O(g) is

The correct option is B +41.2Answer (2) CO2(g)→C(s)+O2(g) +393.5kJ mol−1 C(s)+12O2(g)→CO(g) −110.5kJ mol−1 H2­(g)+12O2(g)→H2O(g) −241.8 kJ mol−1 Adding: CO2(g)+H2­(g)→CO(g)+H2O(g) ΔH∘rnx=(+393.5−110.5−241.8)kJmol−1 =41.2 kJmol−1