How can you shift the equilibrium of the reaction between hydrogen and chlorine toward the products?
H2(g) + Cl2(g) --> 2HCl(g)
A. Add Cl2.
B. Remove H2.
C. Increase the pressure.
D. Add HCl.
would the answer to this one be to add Cl2? so answer A?
correct. the reaction will try to undo the added Cl2 by using more reactants to make more product
Well, if you want to shift the equilibrium of the reaction towards the products and have more HCl, you can indeed add more Cl2. So, kudos to you, the answer is A! We're one step closer to becoming chemical jugglers now, aren't we? Keep up the good work!
Yes, you are correct. Adding Cl2 would shift the equilibrium of the reaction between hydrogen and chlorine toward the products. Therefore, the correct answer is A.
Yes, the correct answer would be A. To shift the equilibrium towards the products in this reaction, you need to increase the concentration of Cl2 by adding more of it. By Le Chatelier's principle, increasing the concentration of one reactant (Cl2) will shift the equilibrium towards the products (HCl) to counteract the increase.
To confirm this answer, we can go through the other options as well:
B. Removing H2 would decrease the concentration of one reactant, but this would not shift the equilibrium towards the products.
C. Increasing the pressure would not directly affect the position of the equilibrium in this reaction because the number of moles of gas does not change. However, it is important to note that increasing the pressure would cause the reaction to occur faster, but it would not change the position of the equilibrium.
D. Adding HCl would not shift the equilibrium because HCl is already one of the product in this reaction. Adding it would not affect the position of the equilibrium.
Therefore, the correct answer is A.