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Heat of Reaction

The heat of f...

Question

The heat of formation of CO $_{(g)}$ and CO $_{2 (g)}$ are $Δ$ H =- 110 and $Δ$ H = -393 kJ.mol $^{- 1}$ respectively. What is the heat of reaction ( $Δ$ H ) (in kJ.mol $^{- 1}$ ) for the following reaction $C O + \frac{1}{2} O_{2} \to C O_{2}$ ?

A

-504

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B

-142.5

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C

-283

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D

504

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Solution

The correct option is C -283
$Δ H_{f}$ of CO $=$ - 110 KJ mol $^{- 1}$

$C (s) + \frac{1}{2} O_{2} (g) \to C O Δ H = - 110 k J m o l^{- 1}$
(i) $C (s) + O_{2} (g) \to C O_{2} Δ H = - 393 k J m o l^{- 1}$

(ii) $C O (g) \to C (s) + \frac{1}{2} O_{2} Δ H = + 110 k J m o l^{- 1}$

Adding (i) & (ii)
$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$

$Δ H = - 393 + 110$ $= - 283 k J m o l^{- 1}$

Option C is correct.

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Similar questions

Q. The heat of formation of

C O (g)

C O_{2} (g)

Δ H = - 110

Δ H = - 393 k J m m o l^{- 1}

respectively. What is the heat of reaction

(Δ H)

m o l^{- 1}

) for the following reaction?

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

Q. Determine whether the reactions with the following

Δ

Δ

S values are spontaneous or non-spontaneous. State whether the reactions are exothermic or endothermic.
(a)

Δ

= - 110

Δ

= + 40 J K^{- 1}

400

Δ

= + 40

Δ

= - 120 J K^{- 1}

250

Calculate the heat of combustion (in KJ) of

methane from the following data

i) C (graphite) + 2H $_{2}$ (g) $\to$ CH $_{4}$ (g), $Δ$ H = -74.8 kJ

ii) C (graphite) + O $_{2}$ (g) $\to$ CO $_{2}$ (g), $Δ$ H = -393.5 kJ

iii) H $_{2}$ (g) +1/2O $_{2}$ (g) $\to$ H $_{2}$ O $(l)$ , $Δ$ H = -286.2 KJ.

Δ H_{f}^{o}

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

H_{2} O_{(g)}

- 393.5, - 110.5

- 241.8

k J . m o l^{- 1}

, respectively. The

Δ H_{f}^{o}

k J . m o l^{- 1}

] for the reaction,

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

Q. Assertion :As temperature increases, heat of reaction also increases for exothermic as well as for endothermic reactions. Because Reason:

Δ

H varies with temperature as given by

{Δ H}_{2} (a t T_{2}) = {Δ H}_{1} (a t T_{1}) + {Δ C}_{P} (T_{2} - T_{1})

.

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