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Activation Energy

What is Δ H...

Question

What is $Δ H$ for the reaction A + B $\to$ C where the mechanism involves several kinetic steps.

A

11 kcal

m o l^{- 1}

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B

4 kcal

m o l^{- 1}

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C

5 kcal

m o l^{- 1}

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D

22 kcal

m o l^{- 1}

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Solution

The correct option is B 4 kcal $m o l^{- 1}$
$Δ H$ = 10 - 6 = 4 kcal $m o l^{- 1}$

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Similar questions

C (s) + O_{2} (g) \to C O_{2}, (g);

Δ H = - 94.3

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

Δ H = - 67.4

O_{2} (g) \to 2 O (g);

Δ H = 117.4

C O (g) \to C (g) + O (g);

Δ H = 230.6

kcal/mol.
Calculate

Δ H

C (s) \to C (g)

Q. The heat of formation of

C_{2} H_{5} O H (l)

- 66 k c a l m o l^{- 1}

. The heat of combustion of

C H_{3} O C H_{3} (g)

- 348 k c a l m o l^{- 1}

△ H_{f}

H_{2} O

C O_{2}

- 68 k c a l m o l^{- 1}

- 94 k c a l m o l^{- 1}

respectively.
Then, the

△ H

C_{2} H_{5} O H (l) \to C H_{3} O C H_{3} (g)

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.3

C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g); Δ H = - 67.4

O_{2} (g) \to 2 O (g); Δ H = 117.4

C O (g) \to C (g) + O (g); Δ H = 230.6

Δ H

C (s)

\to

C (g)

Following are the thermochemical reactions:

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.39

K + H_{2} O \to K O H (a q) + \frac{1}{2} H_{2}; Δ H = - 48.0

K O H + H_{2} O \to K O H (a q); Δ H = - 14.0

The heat of formation (in kcal/mol) of

K O H

Q. Bond dissociation energy of

C H_{3} - H

103 k c a l m o l^{- 1}

and heat of formation of

C H_{4} (g)

- 17.88 k c a l m o l^{- 1} .

The dissociation energy of

H_{2} (g)

H

103 k c a l / m o l .

The heat of formation of methyl radical is ?

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