Study the reaction.
H2SO4(l) + CaCO3(s) ⇌ CO2(g) + H2O(l) + CaSO4(aq)
Which of the following would cause the equilibrium to shift, producing more carbon dioxide gas?
Select all that apply.
removing water from the system
removing H2SO4 from the system
removing carbon dioxide gas from the system (correct)
adding CaCO3 to the system (correct)
a and c are correct. Solids (CaCO3) do not enter into the Keq and I think the question is worded so that isn't a correct answer; however, IF there is enough H2SO4 and CaCO3 is the limiting reagent, then more CaCO3 will increase producing more CO2.
Well, well, well, let's take a look at these options.
First off, removing water from the system. Oh, I see what you're trying to do, you sneaky little equilibrium shifter. By removing water, the reaction is gonna be like, "Hey, where's my water buddy? I need more of that stuff!" So yeah, removing water would indeed shift the equilibrium towards producing more carbon dioxide gas.
Next up, removing H2SO4 from the system. Now, this one is a bit tricky. H2SO4 is one of the reactants, and by removing it, you're basically messing with the balance. The reaction would be like, "Wait, where did my buddy H2SO4 go? I guess I don't need to produce more carbon dioxide gas anymore." So, nope, removing H2SO4 wouldn't shift the equilibrium in the desired direction.
Moving on, removing carbon dioxide gas from the system. Ahh, the classic reverse psychology move. By removing carbon dioxide gas, the reaction is gonna be like, "Hey, hey, we're running out of CO2 here, we should produce more of that!" So yup, removing carbon dioxide gas would indeed shift the equilibrium towards producing more carbon dioxide gas. Bravo!
Lastly, adding CaCO3 to the system. Ah, CaCO3, the comrade of carbon dioxide. By adding more of its pal, CaCO3, the reaction would be like, "Oh, look, more CaCO3, let's convert that into CO2 and have a party!" So yup, adding CaCO3 would definitely shift the equilibrium in the desired direction.
To sum it up, the correct answers are: removing carbon dioxide gas from the system and adding CaCO3 to the system. Good luck with that CO2 production!
To determine which actions would cause the equilibrium to shift and produce more carbon dioxide gas (CO2), we need to analyze the reaction.
H2SO4(l) + CaCO3(s) ⇌ CO2(g) + H2O(l) + CaSO4(aq)
The reaction involves the dissolution of calcium carbonate (CaCO3) in sulfuric acid (H2SO4), resulting in the formation of carbon dioxide gas and calcium sulfate in an aqueous form (CaSO4).
To shift the equilibrium and increase the production of carbon dioxide gas (CO2), the following actions can be taken:
1. Removing water from the system: This will not directly affect the production of carbon dioxide gas because it is not directly involved in the production of CO2.
2. Removing H2SO4 from the system: The reaction requires sulfuric acid (H2SO4) as a reactant, so removing it from the system would hinder the reaction and decrease the production of CO2.
3. Removing carbon dioxide gas from the system: According to Le Chatelier's principle, when a component of the equilibrium mixture is removed, the equilibrium will shift in the direction that produces more of that component. Thus, removing carbon dioxide gas from the system will cause the equilibrium to shift to produce more CO2.
4. Adding CaCO3 to the system: Adding more calcium carbonate (CaCO3) to the system will increase the concentration of the reactant. According to Le Chatelier's principle, increasing the concentration of a reactant will drive the equilibrium towards the products to consume the excess reactant. Thus, adding CaCO3 will cause the equilibrium to shift in the direction of producing more CO2.
Therefore, the correct answers are:
- Removing carbon dioxide gas from the system
- Adding CaCO3 to the system
To determine which factors would cause the equilibrium to shift and produce more carbon dioxide gas, we need to analyze the reaction and understand how different changes can affect it.
In the given reaction between H2SO4 and CaCO3, the forward reaction produces carbon dioxide gas as one of the products. Therefore, any change that favors the forward reaction will result in an increase in the production of carbon dioxide gas.
Let's evaluate each option:
1. Removing water from the system:
Water is a product in the reaction, and removing it would decrease its concentration. According to Le Chatelier's principle, if we decrease the concentration of a product, the equilibrium will shift in the forward direction to produce more of that product. Therefore, removing water from the system would favor the forward reaction, leading to an increase in carbon dioxide gas production. Thus, removing water would cause the equilibrium to shift and produce more carbon dioxide gas.
2. Removing H2SO4 from the system:
H2SO4 is one of the reactants in the reaction. By removing it, we would decrease its concentration, which would favor the reverse reaction. According to Le Chatelier's principle, if we decrease the concentration of a reactant, the equilibrium will shift in the direction that produces more of that reactant. Since the reverse reaction does not produce carbon dioxide gas, removing H2SO4 would not result in increased carbon dioxide production. Hence, removing H2SO4 would not cause the equilibrium to shift and produce more carbon dioxide gas.
3. Removing carbon dioxide gas from the system:
Carbon dioxide gas is one of the products of the reaction. By removing it, we would decrease its concentration. As per Le Chatelier's principle, if we decrease the concentration of a product, the equilibrium will shift in the forward direction to produce more of that product. Therefore, removing carbon dioxide gas would favor the forward reaction, leading to an increase in carbon dioxide gas production. Thus, removing carbon dioxide gas would cause the equilibrium to shift and produce more carbon dioxide gas.
4. Adding CaCO3 to the system:
CaCO3 is one of the reactants in the reaction. By adding it, we would increase its concentration. According to Le Chatelier's principle, if we increase the concentration of a reactant, the equilibrium will shift in the direction that consumes that reactant to restore balance. The forward reaction consumes CaCO3 and produces carbon dioxide gas. Hence, adding more CaCO3 would cause the equilibrium to shift forward, resulting in increased carbon dioxide gas production. Thus, adding CaCO3 would cause the equilibrium to shift and produce more carbon dioxide gas.
Therefore, the correct options are:
- Removing carbon dioxide gas from the system
- Adding CaCO3 to the system