These are examples of Le Chatelier's Principle. There are exotic definitions out there but simple one I've found useful for students is this. "When we do something to a chemical system at equilibrium the system will react to undo what we did to it."
So for number 1, here is the equation.
CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g)
The question is what happens when we add steam. Simple. The reaction will try to undo what we did. We added steam. The system will try to get rid of the extra steam. How can it do that? By using it up. How can it do that? It can shift to the right producing more products and using up the added steam. The end result is that more H2 and more CO are formed and more CH4 and steam are used.
I'll leave #2 for you to do. You need to know one more thing about Le Chatelier's Principle that isn't easy to find. When pressure is increased, the reaction will shift to the side with fewer moles. Or the reverse is when the ressure is decreased, the reaction will shift to the side with more moles. If the number of moles on each side of the equation is the same then pressure changes do not affect the equilibrium so the equation doesn't shift either way.
Use the chemical reaction to answer the question.
CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g)
Which statement best describes the effect of adding more steam to the system?
(1 point)
Adding steam allows more molecules of the products to collide, causing the rate of the reverse reaction to increase.
Adding steam allows more molecules of the reactants to collide, causing the rate of the reverse reaction to increase.
Adding steam allows more molecules of the products to collide, causing the rate of the forward reaction to increase.
Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
Use the reaction to answer the question.
CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy
Which change to the system would be favorable to the forward reaction?
(1 point)
an increase in the concentration of CO
an increase in the concentration of CO2
an increase in pressure
a decrease in pressure
2 answers
1.N2(g) + 3H2(g) ⇄ 2NH3(g)
Which change would happen in the system if the concentration of N2 was increased at constant pressure?
Answer ->The forward reaction would increase to start reducing the concentration of N2.
2.In which situation can Le Chatelier’s principle be applied?
Answer->It can be applied when a reaction is reversible, and environmental conditions are changed.
3. N2(g) + 3H2(g) ⇄ 2NH3(g) + energy
When this reaction has reached equilibrium, how will it respond when the temperature of the system increases?
Answer->The equilibrium will shift to the left.
4. CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g)
Which statement best describes the effect of adding more steam to the system?
Answer->Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
5. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy
Which change to the system would be favorable to the forward reaction?
Answer->an increase in the concentration of CO
Which change would happen in the system if the concentration of N2 was increased at constant pressure?
Answer ->The forward reaction would increase to start reducing the concentration of N2.
2.In which situation can Le Chatelier’s principle be applied?
Answer->It can be applied when a reaction is reversible, and environmental conditions are changed.
3. N2(g) + 3H2(g) ⇄ 2NH3(g) + energy
When this reaction has reached equilibrium, how will it respond when the temperature of the system increases?
Answer->The equilibrium will shift to the left.
4. CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g)
Which statement best describes the effect of adding more steam to the system?
Answer->Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
5. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy
Which change to the system would be favorable to the forward reaction?
Answer->an increase in the concentration of CO
11 answers