Consider the following reaction at equilibrium. what will happen if fes2 is added to the reaction? 4fes2(s) + 11o2(g) ⇜ 2fe2o3(s) + 8so2(g) consider the following reaction at equilibrium. what will happen if is added to the reaction? 4(s) + 11(g) 2(s) + 8(g) the equilibrium constant will increase. the reaction will shift in the direction of the reactants. the reaction will shift in the direction of the products. no change in the position of the equilibrium is observed. the equilibrium constant will decrease.

The reaction will shift in the direction of the products.

Explanation:

According to Le Chatelier's Principle, when a stress is applied to a chemical reaction in a dynamic equilibrium, the equilibrium will shift to counteract the applied stress. FeS₂ is a reactant, so adding more of the reactant will shift the equilibrium to the product side. More of the FeS₂ will get consumed generating more products.

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6