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Hess' Law

The heat of f...

Question

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

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 $- 283$
For $C O$ ,
$C + \frac{1}{2} O_{2} ⟶ C O$ $Δ H_{C O} = - 110$

For $C O_{2}$ ,
$C + O_{2} ⟶ C O_{2}$ $Δ H_{C O_{2}} = - 393$

For the reaction
$C O + \frac{1}{2} O_{2} ⟶ C O_{2}$
We will substract equation 1 from equation 2, we get
$C O + \frac{1}{2} O_{2} ⟶ C O_{2}$ $Δ H_{C O_{2}} - Δ H_{C O} = - 393 - (- 110) = - 283 K J {m o l}^{- 1}$

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Similar questions

Δ H

k J

for the following reaction:

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

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

C (s) + O_{2} (g) \to C O_{2} (g), Δ H = + 94.0 K c a l .

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g), Δ H = - 67.7 K c a l .

From the above reactions find how much heat (Kcal mole

^{- 1}

) would be produced in the following reaction:

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

Q. Consider the following reaction

C (s) + O_{2} (g) ⟶ {C O}_{2} (g) + x k J

C O (g) + \frac{1}{2} O_{2} (g) ⟶ {C O}_{2} (g) + y k J

The heat of formation of

C O (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

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)

.

C (s) + O_{2} (g) \to {C O}_{2} (g); Δ H = r

C O (g) + \frac{1}{2} O_{2} (g) \to {C O}_{2} (g); Δ H = s

then the heat of formation of

C O

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