Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate. (a) Use data in Appendix D to write a balanced equation for the reaction. The reduction product is Mn2+.

Video transcript

Hello everyone today. We have the following problem. Brewing liquid can be created in the laboratory by reacting potassium bromide and meghan ease oxide with a strong acid. If manganese is the reduction product, what is the balanced equation for the reaction? So we have to start by drawing out the half reactions for both of these components. So we'll start with grooming you know, our bromide ion here in the acquis form that is being turned or transitioned into our bro. Mean in the liquid form. And then we also have our mega knees oxide here as a solid. And it is being undergone the process to turn into Manganese two plus in the acquis Since Megan is two plus is the reduction product. Now that we have our half reactions. We must go on to step two. So the step two is to balance oh non oxygen's and non hydrogen. To balance our first equation here, we can simply add a two in front of the bromine, since there are two on the right and now we have an equal number of brahmins. We don't need to add anything to our manganese. The third step we can do is we can balance our oxygen's so we have to balance oxygen's by adding Our water or H 20. So you know, we don't have to do that for our roaming sign. We can skip that stage for our manganese. However, we do have oxygen we need to balance so we see we have one on the left. So we're going to go ahead and leave that manganese oxide as it is. And then we're gonna go ahead and add to this manganese two plus, we're going to add two waters since we have two oxygen on the left and now that is balanced. Next we move on to the fourth stage. After we balance our oxygen's, we balance our hydrogen and we do this by adding H plus ions. And so we see that on our left equation, we don't have to do anything with our bro means. However, for our mega knees equation, we have to go ahead and add some hydrogen. So on the right, we have four hydrogen. So on the left, what we're gonna do as we are going to add, we're going to add four protons or H plus ions on the left. And so now we have an equal number of hydrogen on both sides. The last and final thing that we're going to do is we're going to balance the charges. So next we balance charges by adding electrons. And so what is that going to look like? Well, for our bro mean we are finally going to have to add something to this. So we have our two bromine Aquarius, we have a two coefficient, we multiply it by that negative charge. So we have a negative two charge overall on the left. So that means that we have to add two electrons on the right for our manganese here, we see that we have four plus charge the left and on the right we have a plus two. So what we have to do is we have to add two electrons on the left to help reduce that four plus two A two plus. So we're going to add two electrons to the left and now it is balanced. The charges are balanced. And so now we just simply have to combine our half reactions. And so that's essentially just going to look like. So we're going to have our manganese oxide here Plus our four protons Plus our two bromine ions. And that is going to give us our borough mean Liquid plus our manganese, two plus ions And then two waters over all the electrons of course canceled out the two on the right, canceled out with two on the left. And so it gives us the following chemical reaction as our final answer. And with that we've answered the question overall. I hope this helped. And until next time.