Question

Consider the following balanced thermochemical equation for a reaction sometimes used for H₂S production: 1/8 S₈(s) + H₂(g) → H₂S(g) ΔH = -20.22kj
(d) What is ΔH when 25.0 g of S₈ reacts?

Answer 1

ΔH = -15.78 KJ when 25.0 g of S₈ reacts.

What is Balanced Chemical Equation ?

The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.

The given reaction balanced equation is:

1/8 S₈(s) + H₂(g) → H₂S(g)       ΔH = -20.22kj

Now,

When 1 mol will react, then ΔH = -20.2 × 8

                                                   = -161.6 KJ

When 1 mol of S8 = 8 × 32 g

                             = 256 g

When 256g of S8 react ΔH = -161.6 KJ

When 1 g reacts, ΔH = $\frac{-161.6}{256}$

                                  =- 0.63125 KJ

When 25 g reacts, ΔH = - 0.63125 × 25

                                     = -15.78 KJ

Thus from the above conclusion we can say that ΔH = -15.78 KJ when 25.0 g of S₈ reacts.

Learn more about the Balanced chemical equation here: brainly.com/question/26694427

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