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Entropy

Which of the ...

Question

Which of the following is an example of exothermic reaction ?

A

H_{2} (g) + C l_{2} (g) \to 2 H C l (g); Δ H = - 184.6 k J

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B

N_{2} (g) + O_{2} (g) \to 2 N O (g); Δ H = + 180.8 k J .

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C

C (g r a p h i t e) + H_{2} O (g) \to C O (g) + H_{2} (g); Δ H = + 1314 k J .

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D

C (g r a p h i t e) + 2 S (s) \to C S_{2} (l); Δ H = + 91.9 k J

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Solution

The correct option is A $H_{2} (g) + C l_{2} (g) \to 2 H C l (g); Δ H = - 184.6 k J$
$H_{2} (g) + C l_{2} (g) \to 2 H C l (g)$

$Δ H = - 184.6 k J$
$Δ H$ -ve implies heat will be evolved.

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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

Q. Heat of reaction for the reaction is:

P C l_{5} (g) + H_{2} O (g) ⟶ P O C l_{3} (g) + 2 H C l (g)

P_{w h i t e} + (3 / 2) C l_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ P O C l_{3}; Δ H = - 135.5 k c a l

H_{2} (g) + C l_{2} (g) ⟶ + 2 H C l (g); Δ H = - 44.1 k c a l

P (w) + (5 / 2) C l_{2} (g) ⟶ P C l_{5} (g); Δ H = - 89.6 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (g); Δ H = - 57.8 k c a l

Q. In which of the following reactions, the formation of product is favoured by decrease in temperature?
(1)

N_{2} (g) + O_{2} (g) \to 2 N O (g)

Δ H = 181

2 C O_{2} (g) \to 2 C O (g) + O_{2} (g); Δ H = 566

H_{2} (g) + I_{2} (g) \to 2 H I (g); Δ H = - 94

H_{2} (g) + F_{2} (g) \to 2 H F (g); Δ H = - 541

H_{2} (g) + C l_{2} (g) \to 2 H C l (g)

Δ H = - 44 K c a l

2 N a (s) + 2 H C l (g) \to 2 N a C l (s) + H_{2} (g)

Δ H = - 152 K c a l

N a (s) + \frac{1}{2} C l_{2} (g) \to N a C l (s)

Δ H = ?

Q. Calculate enthalpy for formation of ethylene from the following data:

C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 286.2 k J

C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 1410.8 k J

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