Respuesta :
Answer:
36 KJ of heat are released when 1.0 mole of HBr is formed.
Explanation:
By Hess law,
The heat of any reaction ΔH for a specific reaction is equal to the sum of the heats of reaction for any set of reactions which in sum are equivalent to the overall reaction:
H 2 (g) + Br 2 (g) → 2HBr (g) ΔH = -72 KJ
This is the energy released when 2 moles of HBr is formed from one mole each of H2 and Br2.
Therefore, Heat released for the formation of 1 mol HBr would be half of this.
Hence,
ΔHreq = -36 kJ
36 KJ of heat are released when 1.0 mole of HBr is formed.
The study of chemicals and bonds is called chemistry. There are different types of elements are there and these are metal and nonmetal.
The correct answer is 36 KJ of heat is released when 1.0 mole of HBr is formed.
What is Hess's law?
- The heat of any reaction ΔH for a specific reaction is equal to the sum of the heats of reaction for any set of reactions which in sum are equivalent to the overall reaction:
[tex]H_2 (g) + Br_2 (g) ---> 2HBr (g) \ \ \ \ H = -72 KJ[/tex]
This is the energy released when 2 moles of HBr is formed from one mole each of H2 and Br2. Therefore, Heat released for the formation of 1 mol HBr would behalf on this.
ΔHreq = -36 kJ
36 KJ of heat is released when 1.0 mole of HBr is formed.
Hence, the correct answer is 36KJ.
For more information about Hess law, refer to the link:-
https://brainly.com/question/16759172
