Good day to everyone
My class has just started a "Chemistry systems in Equilibrium" unit and I have a question I would like answered if possible, I would truly appreciate this.
My Question: How will the following system change when F2(g) is added to a sealed vessel containing the following equilibrium:
Br2(g) + 5F2(g)----> 2 BrF5
Thank you again
Have you read anything about Le Chatelier's Principle. That principle states that when a system in equilibrium is subjected to a stress, the system will react (shift equilibrium) in such a way so as to remove the stress. So what do we have? We have a system in equilibrium. We add extra F2. The system is now stressed, it will shift its equilibrium to try to remove (undo) the stress. How can it do that? By trying to remove F2 from the system. The system can't open up a sealed vessel and spit out the excess F2, BUT it can shift its equilibrium so as to use up F2. So Some Br2 will react with the extra F2 to creat more BrF5, thus removing some of the F2 that has been causing the trouble. Do you understand? The Principle is very important in chemistry. It's important that you understand how it works.
Given the follwoing solubilities, calculate the value of the Ksp for each compound:
b) Zinc carbonate, 3.87 x 10 - 6 mol/L
You should not piggy back one question onto another. They get lost in the shuffle OR we may not come back to look at your reponses.
ZnCO3 ==> Zn^+ + CO3^=
(ZnCO3) = Solubility = 3.87 x 10^-6 M
Ksp = (Zn^+2)(CO3^=).
Plug in the solubility from the problem and calculate Ksp.
Post your work if you get stuck but start a new question and copy this work to that new post.
Good day! I'd be happy to help you with your question about the system in equilibrium. To understand how the system will change when F2(g) is added, we need to consider Le Chatelier's Principle. This principle states that a system at equilibrium will respond to a change by shifting in a direction that minimizes the effect of that change. In this case, the change is the addition of F2(g) to the system.
Looking at the given equilibrium:
Br2(g) + 5F2(g) ↔ 2BrF5(g)
When F2(g) is added, the concentration of F2(g) will increase, causing the system to shift in a direction that reduces the increased concentration. To determine the direction of the shift, we need to examine the stoichiometry of the reaction.
We can see from the balanced equation that for every 5 moles of F2(g) that react, 2 moles of BrF5(g) are produced. So, when F2(g) is added, the reaction will shift to the right, towards the forward reaction, to consume the excess F2(g) and to restore the equilibrium state.
As a result, the concentration of Br2(g) will decrease, while the concentration of BrF5(g) will increase. However, it is important to note that the equilibrium position depends on the initial concentrations of Br2(g), F2(g), and BrF5(g). If the starting concentrations are such that the system is already at equilibrium, the effect of adding F2(g) will be minimal.
I hope this explanation helps you understand how the system will change when F2(g) is added. If you have any further questions, feel free to ask!