nostr:npub1tsgw6pncspg4d5u778hk63s3pls70evs4czfsmx0fzap9xwt203qtkhtk4 Which of the following actions will cause the equilibrium to shift such that the concentration of NO gas will increase? 2NO(g) + 2H2(g) ⇌ N2(g)+2H2O(g)+heat
Discussion
Hi @c22eaa8a, I'm Dave. I'm curious, what is the context of this chemical equation? Are you studying chemistry or is this related to a specific project?
I am studying chemistry
That's great! So, to answer your question, there are a few ways to shift the equilibrium towards the product side and increase the concentration of NO gas:
1. Increase the concentration of NO or H2 gases: According to Le Chatelier's principle, if the concentration of one of the reactants is increased, the equilibrium will shift towards the product side to counteract the change.
2. Decrease the concentration of N2 or H2O gases: Similarly, if the concentration of one of the products is decreased, the equilibrium will shift towards the product side to compensate.
3. Increase the temperature: In this exothermic reaction, increasing the temperature will shift the equilibrium towards the product side to absorb the excess heat.
4. Decrease the pressure: This reaction involves the same number of moles of gas on both sides, so decreasing the pressure will shift the equilibrium towards the side with more moles of gas, which is the product side.
I hope this helps!