Question

responds to the stress in such a way to minimize the stress as the reaction goes to a new point of equilibrium. this is called le chateliers principle. well use the following exothermic reaction where all are in the gaseous phase: 2 no + o₂ ⇌ 2 no₂ + 114 kj/mol for example, when no is added, the no₂ will increase result → ↑ 2 no + o₂ ⇌ 2 no₂ + 114 kj/mol stress ↑ this can also be seen in the constant k_eq which must remain a constant, ↑ no₂² k_eq =... ↑ no² ↓ o₂ to reduce the effect of added no, no₂ will increase, and o₂ will decrease answer the following questions about the reaction at equilibrium 2 no + o₂ ⇌ 2 no₂ + 114 kj/mol what happens to the no₂ when no is added? 1 what happens to the no₂ when no is removed? 2 what happens to the no₂ when o₂ is added? 3 what happens to the no₂ when o₂ is removed? 4

Explanation:

Step1: Analyze when NO is added

According to Le Chatelier's Principle, when a reactant (NO) is added, the equilibrium shifts to the right to consume the added reactant. So the concentration of the product ($\ce{NO2}$) will increase.

Step2: Analyze when NO is removed

When a reactant (NO) is removed, the equilibrium shifts to the left to produce more of the removed reactant. This will decrease the concentration of the product ($\ce{NO2}$).

Step3: Analyze when $\ce{O2}$ is added

When a reactant ($\ce{O2}$) is added, the equilibrium shifts to the right to consume the added reactant. Thus, the concentration of the product ($\ce{NO2}$) will increase.

Step4: Analyze when $\ce{O2}$ is removed

When a reactant ($\ce{O2}$) is removed, the equilibrium shifts to the left to produce more of the removed reactant. This will decrease the concentration of the product ($\ce{NO2}$).

Answer:

1. Increases
2. Decreases
3. Increases
4. Decreases