CameraIcon

SearchIcon

MyQuestionIcon

156

You visited us 156 times! Enjoying our articles? Unlock Full Access!

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

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

B

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

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 .

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

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.

Suggest Corrections

thumbs-up

0

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

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Spontaneity and Entropy

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon