Oh the equation is
2 NO2(g) -> N2(g) + 2 O2(g)
and I also thought that the amount of NO2 decreases.
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!!!!!!!!!
1 answer