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
(c) What is ΔH when 2.6 mol of S₈ reacts?

Answer 1

ΔH = -420.16 KJ when 2.6 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,

1/8 mol of S₈ reacts ΔH = -20.2 kJ

1 mol will react ΔH = -20.2 × 8

                                          = -161.6 KJ

2.6 mol will react ΔH = -161.6 × 2.6

                                   = -420.16 KJ

Thus from the above conclusion we can say that ΔH = -420.16 KJ when 2.6 g of S₈ reacts.

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

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