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
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
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.
Well, let's get chemical with these questions!
For the first one, adding steam would increase the concentration of H2O in the system. Since the forward reaction in this case produces the products CO and H2, adding steam and increasing the concentration of the reactant H2O would cause more molecules of the reactants to collide, increasing the rate of the forward reaction. So, the correct answer is: Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
Now, onto the second question! To favor the forward reaction in this case, we want to increase the concentration of the reactants: CO and H2O. This would shift the equilibrium towards the products CO2 and H2. So, the correct answer is: an increase in the concentration of CO.
Hope that brings some chemical humor to your day!
For the first question, adding steam (H2O) to the system will increase the concentration of H2O molecules, which is a reactant in the forward reaction. Therefore, adding steam will cause more molecules of the reactants to collide, increasing the rate of the forward reaction. Thus, the correct answer is: Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
For the second question, to favor the forward reaction in the given chemical equation, it is important to increase the concentration of the reactants or decrease the concentration of the products. Looking at the equation, the concentration of CO is a reactant, and increasing its concentration would shift the equilibrium toward the forward reaction. Therefore, the correct answer is: An increase in the concentration of CO.
To understand the effect of adding more steam to the first chemical reaction, CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g), we need to consider the reaction and the role of steam. In this reaction, methane (CH4) and water (H2O) react to produce carbon monoxide (CO) and hydrogen gas (H2), with the release of energy. This reaction is reversible, meaning it can proceed in both the forward and reverse directions.
When more steam (H2O) is added to the system, it increases the concentration of the reactant water. As a result, more water molecules are available to collide with the other reactants (methane and energy), thus increasing the likelihood of successful collisions. Since the question asks about the rate of the reverse reaction, we can conclude that adding more steam allows more molecules of the reactants to collide, causing the rate of the reverse reaction to increase. Therefore, the correct answer is:
Adding steam allows more molecules of the reactants to collide, causing the rate of the reverse reaction to increase.
For the second chemical reaction, CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy, we need to determine the changes to the system that would favor the forward reaction. This reaction also involves carbon monoxide (CO), water (H2O), carbon dioxide (CO2), and hydrogen gas (H2), with the release of energy.
Increasing the concentration of a reactant or decreasing the concentration of a product usually favors the forward reaction. In this case, an increase in the concentration of CO or a decrease in the concentration of CO2 would tilt the equilibrium toward the forward reaction, as it would increase the number of reactant molecules and decrease the number of product molecules available for collisions. Therefore, the correct answer is:
An increase in the concentration of CO would be favorable to the forward reaction.