What effect does a decrease in the concentration of nitrogen monoxide (no) gas have on the rate of reaction in this chemical equation? 2no(g) + h2(g) → n2o(g) + h2o(g) a decrease in the concentration of nitrogen no and h2 molecules. the rate of the forward reaction blank 1: stabilizes the forward reaction increases the energy decreases the collisions blank 2: remains constant increases decreases

2No(g)  + H₂  → N₂O(g) +H₂O (g)

A decrease  in the concentration  of nitrogen  monoxide   decreases the  collisions  between NO and H₂   molecules.The rate of forward reaction then  decreases

 Explanation

When the concentration  of substance is changed   the equilibrium  shift to minimize  the effect  of that change.

Therefore when  concentration   of  No  (reactant )  is  decreased  the chemical equilibrium  will  shift  toward to reactant side.

This is because there is  less   collision  of  reactant  which led  to formation   of  less product  ( the rate  of forward reaction  decreases)

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

i'm assuming that it's c.) red bank..