Question

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

Answer 1

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

What is Bond Enthalpy?

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:

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