Question

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 monoxide____1____between NO and H2 molecules. The rate of the forward reaction then____2____.

Blank 1:
stabilizes the forward reaction
increases the energy
decreases the collisions

Blank 2:
remains constant
increases
decreases

Answer 1

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)

Answer 2

Answer:

2NO(g) + H2(g) → N2O(g) + H2O(g)

A decrease in the concentration of nitrogen monoxide  decreases the collisions

between NO and H2 molecules. The rate of the forward reaction then decreases .  

Explanation:

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