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vladimir2022 [97]
2 years ago
6

Gases react explosively if the heat released when the reaction begins is sufficient to cause more reaction, which leads to a rap

id expansion of the gases. Use bond energies to calculate ΔH°of each of the following reactions, and predict which occurs explosively:
(b) H₂(g) + I₂(g) → 2HI(g)
Chemistry
1 answer:
iogann1982 [59]2 years ago
3 0

∆H° of the following reaction H₂(g) + I₂(g) → 2HI(g) is -3kJ/mol.

<h3>What is Bond Enthalpy? </h3>

The minimum amount of energy which is required to braak down or form the bonds in chemical reaction is known as bond enthalpy.

It can be calculated as:

∆Hrxn = sum of ∆H bond broken - sum. of ∆H of bond formed.

In order to Calculate ∆Hrxn for the given equation we have:

Bond energies in kJ/mol

  • H—H = 436
  • H—I = 295
  • I—I = 151

Now, the given reaction is

H₂(g) + I₂(g) → 2HI(g)

Here, 1 mol of H₂ and 1 mole of I₂ breaks to form 2 moles of HI.

Therefore,

We know that,

∆Hrxn = B. E(H—H) + B. E(I—I) - 2B. E(H—I)

= 436 + 151 - 2× 295

= 436+ 151 - 590

∆Hrxn = -3kJ/mol.

Thus, from the above conclusion we can say that ∆Hrxn of the reaction H₂(g) + I₂(g) → 2HI(g) is -3kJ/mol.

learn more about Bond energy:

brainly.com/question/26964179

#SPJ4

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