Which of the following is true about the following reaction when an amount of NO₂ (g) is added to the equilibrium reaction? N₂O₄ (g) ⇄ 2 NO₂ (g)
The reaction will shift to the left which will increase N2O5.
Well, let me put on my chemistry hat and tell you a funny story about this reaction. Once upon a time, NO₂ gas walked up to the equilibrium reaction and said, "Hey there, can I join in on the fun?" And N₂O₄, being the friendly compound it is, replied, "Sure thing, come on in!" But little did NO₂ know, by adding more of itself to the mix, it was making N₂O₄ a little nervous. It started to panic, thinking, "Oh no, there's too much NO₂ now! I better counteract this." So, to restore balance, the equilibrium shifted towards the left, forming more N₂O₄ and reducing the excess of NO₂. Therefore, adding NO₂ to the reaction will make the equilibrium shift towards the reactant side, increasing the amount of N₂O₄ and decreasing the amount of NO₂.
When an amount of NO₂ (g) is added to the equilibrium reaction N₂O₄ (g) ⇄ 2 NO₂ (g), the following is true:
1. According to Le Chatelier's principle, when a reactant (NO₂ in this case) is added, the equilibrium will shift to consume the added reactant.
2. In this reaction, adding more NO₂ (g) means increasing the concentration of the reactant. As a result, the equilibrium will shift towards the products side (right) in order to reduce the excess NO₂ and reach a new equilibrium.
3. Consequently, the concentration of N₂O₄ (g) will decrease as it is consumed to produce more NO₂ (g). The concentration of NO₂ (g) will increase due to the added reactant, causing the equilibrium to shift to the right.
4. It's worth noting that the equilibrium constant (Kc) for this reaction remains unchanged since it is based on the ratio of product concentrations to reactant concentrations. Adding NO₂ (g) does not affect the equilibrium constant, only the position of the equilibrium.
Overall, the addition of NO₂ (g) to the reaction will cause the concentration of NO₂ to increase and the concentration of N₂O₄ to decrease, resulting in a shift towards the right to establish a new equilibrium.
When an amount of NO₂ (g) is added to the equilibrium reaction N₂O₄ (g) ⇄ 2 NO₂ (g), the equilibrium will shift to restore the balance between the reactants and products.
To determine which of the following statements is true, we need to consider Le Chatelier's principle, which states that when a system at equilibrium is subjected to a stress, it will adjust in a way that minimizes the effect of that stress:
1. The concentration of N₂O₄ will increase, and the concentration of NO₂ will decrease.
2. The concentration of N₂O₄ will decrease, and the concentration of NO₂ will increase.
3. The concentration of N₂O₄ and NO₂ will both increase.
4. The concentration of N₂O₄ and NO₂ will both decrease.
5. The concentrations of N₂O₄ and NO₂ will not change.
Adding more NO₂ to the reaction increases the concentration of a product. According to Le Chatelier's principle, the system will shift in the direction that reduces the concentration of the product. In this case, the excess NO₂ will react to form more N₂O₄, resulting in a decrease in the concentration of NO₂.
Therefore, the correct answer is:
2. The concentration of N₂O₄ will decrease, and the concentration of NO₂ will increase.