For the reaction 2H2S(g) – 2H2(g) + S2(g), Kc = 9.1x102 at 750 K. What will happen when 0.10 mol of H2S, 1.0 mol of H2, and 1.5 mol of S2 are added
to a 1.0-L container and the system is brought to 750 K?
Nothing; the system is at equilibrium.
More H2S will be formed.
More S2 will be formed than H2.
The amount of H2 formed will be half the amount of S2 formed.
More H2 will be formed than S2.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.