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Crzo/ SFe?t + [4Ht ~6Fest + 2Cr++ 7HzoIn the above redox Icaction, use oxidaton numbers Identify the clement oxidized, the element reduced, thc oxldizing agcnt and ...

Question

Crzo/ SFe?t + [4Ht ~6Fest + 2Cr++ 7HzoIn the above redox Icaction, use oxidaton numbers Identify the clement oxidized, the element reduced, thc oxldizing agcnt and the reducing agent_nannd of the element oxidized:name of the clcment reduced:formula of the oxidizing agent:formula ofthe reducing agent:

Crzo/ SFe?t + [4Ht ~6Fest + 2Cr++ 7Hzo In the above redox Icaction, use oxidaton numbers Identify the clement oxidized, the element reduced, thc oxldizing agcnt and the reducing agent_ nannd of the element oxidized: name of the clcment reduced: formula of the oxidizing agent: formula ofthe reducing agent:



Answers

For the redox reaction $3 \mathrm{Mn}^{2+}+2 \mathrm{HNO}_{3}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow$ $3 \mathrm{MnO}_{2}+2 \mathrm{NO}+6 \mathrm{H}^{+},$ assign oxidation numbers and use them to identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent.

So doing the once over on this question, you can tell that um something that has a reaction with things in elemental form is likely going to be your redox reaction. And if you go back and you look at all of the oxidation numbers for everything. So, for instance, sodium here is a plus one oxygen and negative two hydrogen plus one, you have another plus one hydrogen. The cost versus the plus five. The oxygen is a negative too. Here we have plus one plus one plus five, negative two plus one minus two. The oxidation numbers all stayed the same for all of the elements. So this is not a redox reaction. In fact, this is an acid base neutralization reaction. Then for B we've got a plus one for hydrogen and negative three for nitrogen, oxygen is a negative to carbon is a plus four. Here, oxygen is a negative two hydrogen is a plus one nitrogen, here is the negative three hydrogen is a plus one, we have a plus one plus four minus two for carbon and oxygen. This is also not a redox because all the oxidation numbers stayed the same, then indeed you have plus one minus one plus one plus one plus six minus two, plus one minus one plus one minus two plus six. Again, none of the oxidation numbers changed. This is also not a redox reaction. If you look at the oxidation numbers here in C we have elemental form magnesium and titanium, so those are zero. Here, magnesium is a plus to hear the chlorine is a minus one. Now, if you take a look, you will see that the titanium went from a plus 4 to +80. So that means that there was a reduction. It was gaining electrons. So that means that your T. I plus four in that ionic compound was reduced. And that means that it would be known as the oxidizing agent. It oxidizes the other reactant. And then you'll notice that your magnesium went from zero to a plus two. So that means that there was a loss of electrons. So the magnesium is oxidized and this would be called the reducing agent because it reduces the other reactant.

They were given certain chemical reactions, a certain chemical reaction. We have H plus reacting with pro magnet and iron ions. And we have the following net chemical reaction. So we're asked to assign oxidation number. So for hydrogen, just the charge plus one, oxygen is always almost always -2. So in order to balance out charge, mint, magnesium plus seven, this is just plus two according to the charge plus three, according to the charge Plus two according to the charge oxygen almost -2, always plus one for the hydrogen to balance out the charge on the oxygen. So this gives our different oxidation states. So we can see here that essentially iron izaak supply oxidized from a plus two two plus three oxidation state. So F E two plus is oxidized and pro magnet is reduced from M nine plus 72 Mn two plus 22 plus. So this is reduced. So the oxidizing agent, uh the oxidizing agent is the agent that's going to lead to oxidation itself is not oxidized itself, and the reaction is actually reduced. So this is the oxidizing agent. And the reverse would be true for the reducing agent, which would be the folly. And this gives our final answer.

In Problem 28. For the Redox reaction, assign observation number. Identify the element oxidized the element reduced oxidizing agent and reducing agent. So this question is taken from the topic Oxidation reduction, Redox reaction and the concept behind this question is the oxidation reduction oxidizing agent and reducing agent. So first off, all we try to understand the term oxidation. So oxidation means laws off electrons or in terms off the oxidation number. We can be finance. Oxidation is the increase in oxidation number. So oxidation number is basically the charge assigned often element when present in combined state with other items, or has in its own form, according to some set off role, and that will are called the oxidation number rules. Now we can define the reduction, so reduction is gain off electrons or in terms off the oxidation number. We can defend us decrees in oxidation number. So our redox reaction is direction in which both oxidation and reduction take place simultaneously. So this type off reaction, in which both oxidation and reduction take place so that are called the Redox reaction. So now we can define the term oxidizing agent and reducing agent. So now let us understand the term oxidizing agent. So oxidizing agents are those species which can oxidize other but itself reduce. Okay. And the next time is the reducing agent. So reducing agents are those species which can reduce other but itself oxidized. Okay, so now coming to the question that is okay, the given Redox reaction. So this is the redox reaction that is Cuban in the question. First we find out the oxidation number off each element in this Redox reaction. Okay, so the oxidation number off sulfur in Salford I own is plus six. Oxygen is minus two nickel two plus ions plus two sulfur in sulfur dioxide is plus for oxygen is minus two and nickel in case off. Nickel oxide is blissful and oxygen is minus two. So now we can see that the sell for in this case is reduced. So that means the reduction in this case and nickel is oxidized. So oxidation can take this in the case off nickel. Okay, so now we can see that the we can find out the oxidizing agent introducing agents oxidizing agent means which can oxidized other but itself reduced. So that means this can act as theocracy arising agent And this can act as the reducing agent because in case off oxidizing agent, which can oxidize the other. So now we can see that this nickel is oxidized and sulfur in this case is reduced. So that is why this self it I own can act as the oxidizing agent and in case of reducing agent, which can reduce other So, uh, the cell for the cell phone is reduced and itself is oxidized. So nickel is oxidized in this case. So overall, we can see that as the oxidation number off nickel increase from plus Toto plus four. So it is oxidized and hence a call to plus ion act as producing agent as the oxidation number, sulfur degrees from plus four to plus six to plus four so it is reduced. And hence actors and Salford ion act as the oxidizing event

Okay, so for number seven, let me change the color here. F E, N B R two or an elemental form B R. Is a negative one in the compound, F E. Is a plus too. If you're going from zero to plus two, that means that's a loss of electrons. So that means that this is oxidized. So this would be the reducing agent and then browning is going from a zero to a negative one, that's a gain of electrons. So this is reduced. So we would call it the oxidizing agent. Then on B, we've got a plus one on hydrogen and negative one on iodine, plus one on the H two, S. H and H two. S. +04 negative two on the oxygen. To figure out the sulfur, we've got two hydrogen at a positive one plus sulfur plus negative eight on the oxygen adds up to the neutral compound, which is zero. So if we're going to end up being a plus six here, then here we've got plus one on the H and H two S, negative two on the sulfur, elemental iodine. So that's zero. Oxygen is a negative two hydrogen as a plus one. Then you've got your id I'm going from a negative 1-0. So that's going to be a loss of electrons. So that means that this is oxidized. We would call this the reducing agent and then you've got your sulfur going from a positive six to a negative two. That's a gain an electron. So that means it is reduced and we would call this the oxidizing agent, then in C you've got hydrogen peroxide. So it's a plus one on the hydrogen and minus one on oxygen mono atomic ion, which is the same as its charge, plus two oxygen. Here is a negative two hydrogen as a plus one mono atomic ion, same as its charge, which is plus three negative two on oxygen plus one on hydrogen. If he goes from a plus two two plus three, that means this is a loss of electrons. So that means this is oxidized. We would call this the reducing agent and then you've got this oxygen going from a negative one to a negative two. That's a gain an electron. So this is reduced and we would call this the oxidizing agent.


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