Question

consider the reaction of production of nitrogen monoxide from nitrogen and hydrogen: n₂(g) + o₂(g) ⇌ 2no(g). the reaction is endothermic in the forward direction. drop each type of disturbance in the correct category. causes the concentration of no to increase and the concentration of n₂ and o₂ to decrease as the result of the equilibrium shift causes the concentration of no to decrease and the concentration of n₂ and o₂ to increase as the result of the equilibrium shift adding n₂ adding o₂ removing o₂ adding no removing n₂ removing no heating up the reaction mixture cooling down the reaction mixture

Explanation:

Step1: Recall Le - Chatelier's principle

Le - Chatelier's principle states that a system at equilibrium will shift to counteract any applied stress. For an endothermic reaction $N_2(g)+O_2(g)
ightleftharpoons 2NO(g)$, heat is a reactant in the forward - direction.

Step2: Analyze adding $N_2$

Adding $N_2$ increases the concentration of a reactant. The system will shift to the right (forward direction) to consume the added $N_2$. This causes the concentration of $NO$ to increase and the concentration of $O_2$ to decrease.

Step3: Analyze adding $O_2$

Adding $O_2$ increases the concentration of a reactant. The system will shift to the right (forward direction) to consume the added $O_2$. This causes the concentration of $NO$ to increase and the concentration of $N_2$ to decrease.

Step4: Analyze removing $O_2$

Removing $O_2$ decreases the concentration of a reactant. The system will shift to the left (reverse direction) to produce more $O_2$. This causes the concentration of $NO$ to decrease and the concentration of $N_2$ to increase.

Step5: Analyze adding $NO$

Adding $NO$ increases the concentration of a product. The system will shift to the left (reverse direction) to consume the added $NO$. This causes the concentration of $N_2$ and $O_2$ to increase and the concentration of $NO$ to decrease.

Step6: Analyze removing $N_2$

Removing $N_2$ decreases the concentration of a reactant. The system will shift to the left (reverse direction) to produce more $N_2$. This causes the concentration of $NO$ to decrease and the concentration of $O_2$ to increase.

Step7: Analyze removing $NO$

Removing $NO$ decreases the concentration of a product. The system will shift to the right (forward direction) to produce more $NO$. This causes the concentration of $N_2$ and $O_2$ to decrease and the concentration of $NO$ to increase.

Step8: Analyze heating up the reaction mixture

Since the forward reaction is endothermic, heating up the reaction mixture (adding heat) is like adding a reactant. The system will shift to the right (forward direction). This causes the concentration of $NO$ to increase and the concentration of $N_2$ and $O_2$ to decrease.

Step9: Analyze cooling down the reaction mixture

Since the forward reaction is endothermic, cooling down the reaction mixture (removing heat) is like removing a reactant. The system will shift to the left (reverse direction). This causes the concentration of $NO$ to decrease and the concentration of $N_2$ and $O_2$ to increase.

Answer:

Causes the concentration of NO to increase and the concentration of $N_2$ and $O_2$ to decrease: adding $N_2$, adding $O_2$, removing $NO$, heating up the reaction mixture
Causes the concentration of NO to decrease and the concentration of $N_2$ and $O_2$ to increase: removing $O_2$, adding $NO$, removing $N_2$, cooling down the reaction mixture