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Question 12The balanced equation for an oxidation- reduction reaction taking place in aqueous solution is 3 CzOa 2 (aq) 2 MnO4 (aq) + 4 OH" (aq) 76 CO3 (aq) 2 ...

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Question 12The balanced equation for an oxidation- reduction reaction taking place in aqueous solution is 3 CzOa 2 (aq) 2 MnO4 (aq) + 4 OH" (aq) 76 CO3 (aq) 2 MnOz (s) 2 Hzo (€)1.2 moles of MnOa is converted to 2 moles of MnOz by losing 6 moles of electrons: II: pH of the solution decreases as the reaction proceeds. III: C2O4 2- is the reducing agent:Which of the given statements is/are true for this reaction?Your answer:Only IIIand IIIl and IlIL,ll, and IIIOnly '

Question 12 The balanced equation for an oxidation- reduction reaction taking place in aqueous solution is 3 CzOa 2 (aq) 2 MnO4 (aq) + 4 OH" (aq) 76 CO3 (aq) 2 MnOz (s) 2 Hzo (€) 1.2 moles of MnOa is converted to 2 moles of MnOz by losing 6 moles of electrons: II: pH of the solution decreases as the reaction proceeds. III: C2O4 2- is the reducing agent: Which of the given statements is/are true for this reaction? Your answer: Only III and II Il and IlI L,ll, and III Only '



Answers

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions.\begin{equation}
\begin{array}{c}{\text { (a) } \mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad{\quad 4 \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+10 \mathrm{HCl}(a q)}\end{array}
\end{equation}
\begin{equation}
\begin{array}{l}\quad\quad\quad\quad\quad\quad{\text
{ (b) } \mathrm{Br}_{2}(l)+2 \mathrm{K}(s) \longrightarrow 2 \mathrm{KBr}(s)} \\\quad\quad\quad\quad\quad\quad {\text { (c) } \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)}\end{array}
\end{equation}
\begin{equation}
\begin{array}{r}\quad\quad\quad\quad{\text { (d) } \mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+} \\ {2 \mathrm{NaCl}(a q)}\end{array}
\end{equation}

We'll be looking at to the complete was four completely. Ducks equals equations and we will be one finding the to half the actions, the each and two. We will be finding the oxidizing agent involved, and clearly we'll be finding the reducing agent involved. So the first of really docks equation will be too stoned, impossible to yields to stroll into oxide. So since these two wasn't elemental male, it states the each average wages you. But in this compound study, um, has a two plus charge in Austin. Have a to minus charge. So when we look at the oxidizing, half the action and the reducing deduction have the action, we'll find that still on him is oxidized since it gains new luck turns. Um, since all the coefficients can be divided by two, we will be doing just that and for the reduction of question will go to plus four U minus. Yields to O to minus with the oxidizing needn't as oxygen, since it is what is adduced and the introducing agent as Dylan team, which oxidize so for the second completely docks equation, we have to with him plus Midge to Gus meals to Ally These are the ones the gun industry ended. States, I have a plus one charge. I didn't have a plus minus one charge. Now we can let out by half reactions. Knock those oxidation. Have the action is lift them yields. Let them plus plus one. A lot done. Since we started off with to elect owns two lithium Adams. We would technically have to before the each of these parts of the equation. But since the all balance hope, it's just one gust. Boyd, Time for the doctor. Have a question we have to which to were aged two plus tu minus yields to huge minus. So now we have the huh oxidizing agent as hydrogen, where the owner that's reduced and me reducing agent as lithium boiled element that is oxidized and the next completely docks. The action is to caesium. Plus, we are too heels to see us b horror. Once again, these in the standard states he's a mother plus one charge of them has a minus one charge. So the half of the actions we have caesium to seize to just cesium meals caesium plus plus one electron and two plus two fields to the uh, minus. Would the oxidizing you don't has? And the the Duce Nu agent caesium. So on final completely leader, the docks and the action is the American Museum plus, like to June yields like museum, too. From this weekend, we know that magnesium have a two plus the nitrogen has three minus charge and we can I have half the actions as fall wounds. The oxidation reaction will be doing magnesium build stilling magnesium to plus plus six electrons. Let's in. All of these cowfish is indivisible by three. We will simply say that that's magnesium, magnesium to both plus two tons and for the reduction of question. Dejan plus six u minus meals to nitrogen three minus with our Bach said, dies in agent as my Children. And, uh, the do sing agent has magnesium.

This question is going to take a look at an important chemical process or type of reaction called a redox reaction or oxidation. And reduction. And going to look at this with respect to a couple of different examples here. So the first example we're going to take a look at is going to deal here with a methane and reacting with uh water. So there should be a two there. So methane is going to react with water to form carbon monoxide and hydrogen gas. And one way that you can identify whether an oxidation reduction has taken place in reaction is look at what happens to the bonding between a species and oxygen. So if we look at what happens to methane, more specifically, the carbon and methane, it loses bonds to hydrogen and as a product gains a bond to oxygen or gains a triple bond, the oxygen, but in any case it's gaining bonds to oxygen throughout the course of the reaction. Whenever something gains bonds to oxygen, it has been oxidized or it's undergone oxidation. So methane has been oxidized here. So any time we talk about oxidation, it's a loss of electrons. So where do those lost electrons go? Um they have to go then to the water. And if we look at what happens to the hydrogen, specifically in the water molecule as it progresses throughout the reaction, it loses bonds to oxygen to become hydrogen gas. And any time also, we see a loss of bonds, oxygen just as gaining of bonds to oxygen means oxidation is taking place. If we lose bonds to oxygen, that means the species has undergone reduction and so water here is reduced or undergoes reduction, It's the species that's reduced. A couple of other terms. You should be familiar with oxidizing agent, reducing agent. So an oxidizing agent is always the thing that gets reduced throughout the course of a reaction. So who is reduced? Water? Therefore water is our oxidizing agent. In this example, a reducing agent gets oxidized. Who is oxidized? Methane was therefore methane is the reducing agent in this example. In the second example, we're looking at a silver nitrate and copper reaction here and here. It it kind of is a little more useful to look at assigning oxidation numbers to be able to see where the electrons are transferred in this reaction. So, copper, in its elemental form has an oxidation number of zero. Throughout the course of the reaction, it becomes copper nitrate nitrate ion has a minus one charge, and since there are two of them, they contribute -2 overall to the molecule. So copper then has a plus to charge in the copper nitrate molecule. So any time there's an increase in oxidation number. Throughout the course of the reaction, from reacting to product, copper goes from zero two Plus 2. That's an increase in oxidation number. That's a sign that oxidation has taken place. Therefore copper is oxidized in this reaction. And if we go to our terminology, a pure oxidizing or reducing agent. Ah but you can see here, okay, the thing that gets oxidized is are reducing agent. Therefore, since copper is oxidized, it is the reducing agent in this example. How about the silver? Alright, the silver goes from a plus one charge in the silver nitrate ion too. Remember copper was zero in its elemental form. So silver in its elemental form will be zero. Check it out guys. We see a reduction in the oxidation number. It's reduced from a plus one to a zero C. The terminology whenever something is has a lower oxidation number or state in the product form than it had in the reactant form. That's evidence that reduction has taken place. Therefore, silver and the silver nitrate has undergone reduction. Copper went underwent oxidation. So silver and the silver nitrate um underwent reduction and anything that's reduced throughout the course of a reaction is are oxidizing agent. So, silver nitrate in this example is our oxidizing agent. Now that you're catching on, I'm not going to spend as much time in the last two examples. But let's take a look at two more and follow the same ideas. This is zinc reacting with hydrochloric acid. So zinc starts out as a zero for its oxidation state, it becomes zinc chloride and it takes on a plus to oxidation state. What do we know? An increase in oxidation number means zinc has been oxidized the hydrochloric acid, The hydrogen goes from a plus one oxidation number two, Elemental zero anytime we see a reduction in oxidation number from plus 1 to 0 here, that's reduced. The zinc chloride then is reduced whose are oxidizing and reducing agent. Again, the thing that gets oxidized is are reducing agent. And the thing that gets reduced in this case, the hydrochloric acid, these are oxidizing agent. One final example, Um here we're going to look at the chrome eight and hydrogen ions, or protons. And so um if we identify here what's going on throughout the course of the reaction, it's a little bit of a trickier example. But let's look at what happens to the chromium whenever you see transition metals in a compound, especially when they're combined with oxygen, you want to think of um an oxidizing agent and you want to monitor what happens to that transition metal. So in this case, each of the oxygen is going to contribute -2 and have a -2 oxidation number four of them contribute -8 overall. And if we look at and you know, something wasn't right here, this should be a tu minus charge on the chrome eight. So, um in order to have an overall minus two charge, that means the chromium has to have a plus six. So plus six plus the minus eight gives that minus two charge that we expect on the chrome eight ion. Now, what happens to the chromium as it becomes a product, the same thing here, look at the oxygen minus two For each of the oxygen's, but there are seven of them. So all together they contribute -14. So in order to get a -2 overall charge in the Dike Romain Ion. And since I have two chromium, each of the chromium is has to have a plus six church Plus six times 2 is plus 12, 12 plus negative 14 gives the negative to charge on the dike Romanian. And look, there's been no change in oxidation number for the chromium. There's been no change in oxidation number for the other species, either the hydrogen or oxygen. So in this example, this is not a redox reaction because oxidation or reduction has not taken place on any of the reactant is involved.

So the first part of the question is asking which of the following are Redox reactions? Redox reaction, by definition, means that something gets oxidized and something else gets reduced. So let's take a look at each option. First will determine the oxidation states of each element, and whether or not it changes in the reaction before we start, let's take a look at the table on the right hand side, and it gives us a general idea, UH, the rules of oxidation states. So Group One elements will have an oxidation state of plus one group. Two elements plus two Hydrogen will be plus one when it's bonded to non metals and negative +11 responded to metals. Florian will always be negative. One oxygen will be in negative to unless it's bonded to Florian or to another. Oxygen and chlorine will be negative one, unless it's bonded toe florian or oxygen because they're more electronica. So let's get started. Magnesium here will be plus two because it's a group to element, and the oxygen will be negative, too. The vision here will be plus one oxygen will be negative, too negative. Two types freeze negative six, and we have to Hydrogen is here, so the carbon will have to be plus four. In order to give us an overall charge of zero for this compound, magnesium here again will be plus two. The oxygen will the negative to know we calculate a gun negative two times three is negative six plus two. So the carbon will have to be plus four for in overall charge again zero and then the oxygen here will be negative two and hydrogen is plus one. You know, we have to. Hydrogen is so plus to a negative to a zero. So if we take a look at all the elements in this reaction, we'll see that none of them have a change in oxidation states. Magnesium remains that plus two oxygen is negative. Two hydrogen is plus one and carbon is plus four. So this is not a redox reaction because nothing has been reduced or oxidized removal. Depart be for potassium. It will have oxidation state of plus one because it's a good one element. Oxygen will be negative to negative. Two times three is negative. Six. So in this case, the nitrogen will have to be plus five in order to give us over all charges. Euro potassium here again will be plus one. Oxygen will be negative, too. And here we have two oxygen's instead of three. So negative two times two. That's a negative four, and we have one potassium. So the Nigerian will have to be plus three in this case to balance it out and give us a charge of zero overall and oxygen here. Because there is no charge, then it has an occupation state of zero. So in this reaction we can see that oxygen has been oxidized, which means it has lost electrons, and it is also a reducing agent because it had reduced the nitrogen. Nitrogen here has gained two electrons they went from plus five two plus three. So it's going to electrons. That means it's been reduced, and a good way to remember that is because it goes from plus five two plus three. So the number has been refused, so lettering has been reduced, which means it's an oxygenating agent because it made oxygen to be oxidized. Moving on to part three, the hydrogen here has a no overall charge of zero. The oxygen will be negative two and the copper. We'll have to be plus two in order to balance it out here. Copper is on its own with no overall charge. So it's zero. Oxygen here is negative two and then the hydrant is plus one. So here we can see that the hydrogen went from zero to plus one. So it's been oxidized. It lost that electron, and we would also say it's the reducing agent because it reduced copper. Copper has been reduced. It gain two electrons and copper would be the oxidizing agent. Moving on to D for sodium. Here it has oxidation state of plus one because it's a group one element, oxygen is negative. Two and hydrogen this plus one. So all these numbers will balance out to zero hydrogen here. This plus one chlorine is negative. One again on this side. Saudi movie plus one Chlorine negative one. Oxygen is negative two and hydrogen this plus one. And in this case, we can see that none of thes elements have have had a change in their oxidation states. So sodium stays at plus one oxygen negative too. Hydrogen plus one and chlorine is negative one. So this is not a redox reaction and low for either the hydrogen will be zero because there is no charge. Chlorine again, it'll be zero because it has no charge. And here the hydrogen will be plus one and the chlorine minus one. So here we would say the hydrogen has been oxidized and it is the reducing agent. And then the chlorine has been reduced because it gained one electron and it's the oxidizing agent. Then the loss part you the oxygen here will be negative to negative two types series negative six. And this compound has an overall charge of zero, so the sulfur would have to be plus six Did violence that owned the oxygen is negative. Two on the hydrogen is plus one, but and then we go over to the side. Heidrun again will be plus one. Oxygen is negative to negative. Two times for is negative eight and we have to hydrants here. So the sulfur would have to be plus six in order to give us an overall charge of zero. So this is not a redox reaction, because nothing has been oxidized

In order to identify a chemical reaction as a Redox reaction, we need to see a change in the oxidation state. If the oxidation state increases, then it was oxidized and it served as the reducing agent. If the oxidation state was decreased, it was reduced and it served as Theo Oxidizing agent. Here we have several chemical reactions, six of them the first one. It's this one shown here in order to determine whether or not this is a Redox reaction. Let's first assign oxidation, states oxidation. States will correspond to the charge if we have an ionic compound. Here we have magnesium oxide where magnesium has a two plus charge, so it has a plus to oxidation. State and oxygen with a minus two charge has a minus two oxidation state remembering our oxidation state rules. Oxygen is typically negative. Two. Hydrogen is typically plus one. When we put in the negative to in the plus one, we've got negative two times three, which is negative six and then plus one times two, which is plus two. So that then gives us carbon as a plus four. Well, then go to the magnesium here, magnesium carbonate and magnesium with the two plus charge. So we've got a plus to oxidation State oxygen is minus to this whole thing. Carbonate has a minus two charge. So the some of the oxidation states needs to equal minus two. For that to occur, carbon needs to be plus four and then for water. We've got minus two and plus one. If we look closely, there is no change in oxidation state of any element because there's no change in oxidation state of any element. This is not a redox reaction. The next one we have potassium nitrate going to potassium nitrite and oxygen will assign oxidation. States, oxygen is minus two. Potassium is plus one Nitrogen is going to be the minus two, multiplied by three is minus six plus one. So what's left would be plus five in order to get this to be somewhat to zero. Then when we go over to potassium nitrite, got minus two on oxygen plus one on potassium, so that gives us minus four and a plus one. So this needs to be plus three and oxygen elements by themselves in their elemental form, have an oxidation state of zero. So we now see that nitrogen went from plus five two plus three, so it was reduced and oxygen went from minus 2 to 0, so it was increased. It was oxidized. The potassium nitrate is serving as both the oxidizing and the reducing agent. Normally, when we defined the agent, it's the entire compound. However, some teachers might suggest that the agent is going to be the element within the compound. But it's more correctly to describe the agent as an actual chemical. That is, that is part of the chemical reaction. So we would say that potassium nitrate is serving both as theocracy izing and the reducing agent. This is often this often occurs with many redox reactions. The next reaction is hydrogen gas, with copper to oxide going to copper metal on water. Hydrogen gas is an element by itself, so it has an oxidation state of zero. Oxygen has a minus two charge, so it has a minus two oxidation state and copper as a plus to charge, so it has a plus to oxidation state copper by itself. Here is zero, and then the water oxygen's minus two and hydrogen is plus one, so we see that hydrogen has a change in oxidation state of zero to plus one. So it increased. So it was oxidized and copper goes from plus 2 to 0. So it decreased, so it was reduced. So we would say that hydrogen gas is the reducing agent, and copper to oxide is the oxidizing agent. For the next one, we have sodium hydroxide reacting with hydrochloric acid producing sodium chloride and water sodium has a plus one charge. So it has a plus one oxidation state hydroxide. Oxygen hydroxide is minus two. The hydrogen is plus one. They all some up to zero. Hydrogen is gonna be plus one. So to sum, up to zero chloride needs to be minus one. So dems plus one because that's his charge. Chlorides minus one because that's its charge. And then hydrogen and hydrogen typically being plus one and oxygen typically being minus two. We look closely. We see that there is no change in oxidation state of any element present. So this is not a redox reaction. The next one is hydrogen gas with chloride gas going to hydrogen chloride. Hydrogen by itself as an element in its pure form, has an oxidation state of zero chlorine gas, an element by itself has an oxidation state of zero. But when we form hydrogen chloride, hydrogen with plus one and chloride will be minus one similar to what we had up here. We do see a change in oxidation state are hydrogen goes from zero to plus one. So it was oxidized and chlorine goes from zero to minus one. So it was reduced. So we can say that hydrogen being oxidized is the reducing agent and chlorine being reduced is three oxidizing agent, the last one. We have sulfur trioxide reacting with water producing sulfuric acid. Oxygen has minus two tu minus two times three minus six. So sulfur needs to be plus six water will be have its oxygen minus two in its hydrogen plus one. Then we go to sulfuric acid. Oxygen will be minus two or four of them, so that's minus eight and then plus one times two. So we're now down to negative six. So that means sulfur needs to be plus six. And again, looking closely, we see no change in oxidation states of any of the elements. Therefore, this is not a Redox reaction


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