Question

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.

Answer 1

 4FeS₂ + 11O₂ →  2Fe₂O₃  +8SO₂

What  happen  if  FeS₂  is added  to the reaction  is that

The reaction will shift  in the direction  of the products

Explanation

• FeS₂  is  a reactant  in reaction above .

• When  more  of reactant  added  to  a system at equilibrium,    it increases the concentration  of  reactant molecules.

• According to collision theory,this  increase   the number of collisions per second  of reactant  molecule  and therefore more product is formed.

Answer 2

Answer:

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.