2 NO2(g) N2(g) + 2 O2(g)
The ¥ÄH¡Æ for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if NO2 is added to the reaction mixture at constant temperature and volume? (Select all that apply.)
And here's the options.
The reaction absorbs energy.
The reaction releases energy.
[NO2] increases.
[NO2] decreases.
[NO2] remains constant.
[N2] increases.
[N2] decreases.
[N2] remains constant.
[O2] increases.
[O2] decreases.
[O2] remains constant.
What I thought was:
Since the number of reactant is increased, the reaction will shift to the right. Therefore, the product, which is N2 and O2 will increase and it will release heat because it is exothermic reaction.
I tried several times and I still get wrong.
Help me!
And thank you alot!!!!!!!!!
Oh the equation is
2 NO2(g) -> N2(g) + 2 O2(g)
and I also thought that the amount of NO2 decreases.
Based on the given reaction and the change in enthalpy (∆H) of -66.4 kJ, we can determine the following:
1. The reaction releases energy: Since the ∆H value is negative, it indicates that the reaction is exothermic, releasing energy.
2. [NO2] increases: If NO2 is added to the reaction mixture, the concentration of NO2 will increase, as more reactant is being added.
3. [NO2] remains constant: Since NO2 is being added to the reaction mixture, the concentration of NO2 will not decrease, but rather increase.
4. [N2] increases: As the reaction shifts to the right, more N2 will be formed, causing the concentration of N2 to increase.
5. [N2] remains constant: The concentration of N2 will not decrease, but it will definitely increase due to the addition of NO2.
6. [O2] increases: As the reaction shifts to the right, more O2 will be formed, leading to an increase in the concentration of O2.
7. [O2] remains constant: The concentration of O2 will not decrease, but it will definitely increase due to the addition of NO2.
To summarize, the correct answers are:
- The reaction releases energy.
- [NO2] increases.
- [N2] increases.
- [O2] increases.
Based on the given reaction and information, let's analyze the situation step by step:
1. The reaction is represented as:
2 NO2(g) -> N2(g) + 2 O2(g)
2. The ΔH° for the reaction is -66.4 kJ, which indicates that the reaction is exothermic (releases energy).
Now, let's consider the effect of adding more NO2 to the reaction mixture at constant temperature and volume:
1. Adding more NO2 increases the concentration of the reactant NO2. Since an increase in reactant concentration typically shifts the equilibrium towards the products, it suggests that the equilibrium will shift to the right (towards N2 and O2).
2. As a result of the equilibrium shift to the right, the concentrations of the products, N2 and O2, are expected to increase.
3. Since the reaction is exothermic (ΔH° = -66.4 kJ), it means that the reaction releases energy. Adding more reactant NO2 will favor the forward reaction and shift the equilibrium to the right, releasing even more energy.
Based on this analysis, the correct choices would be:
- The reaction releases energy.
- [NO2] increases.
- [N2] increases.
- [O2] increases.
It's important to note that the concentrations of NO2, N2, and O2 will change, and the overall energy of the system will decrease (as energy is being released).