Initially the following reverseable reaction is at equilibrium. CH 4(g) +2O 2(g)
ID: 866550 • Letter: I
Question
Initially the following reverseable reaction is at equilibrium.
CH4(g) +2O2(g) ? CO2(g) + H2O(l)
If equilibrium is disrupted, describe what would happen to the concentration of the given chemical once the system returns to equilibrium.
A). Increases B). Decreases C).No Change
1. When CO2(g) is added, what happens to the concentration of H2O(l)?
2. When H2O(l) is added, what happens to the concentration of CO2(g)?
3. When CH4(g) is added, what happens to the concentration of O2(g)?
4. When CH4(g) is added, what happens to the concentration of CO2(g)?
5. When H2O(l) is added, what happens to the concentration of H2O(l)?
6. When CH4(g) is added, what happens to the concentration of H2O(l)?
Explanation / Answer
1) Is you add CO2, the equilibrium shifts to reactants, PRoducts will decrease. H2O decreases (B)
2) When H2O is added, the same happens as in 1). CO2 will decrease (B)
3) If you add CH4 there will be an excess of reactants, the shift goes to products, O2 must decrease (B)
4) If you add CH4, as said before, the shift goes to products, CO2 must increase (A)
5) If you add H2O is added, the products will be a lot, eventually the equilibrium will produce more reactants and will lower, decrease the H2O. Choose B
6) Ify ou add CH4, the shift goes to products, then H2O will increase, choose A