determine-which-of-the-reactions-in-exercise-5-is-not-a-redox-reaction-explain-your-reasoning-2

Name: determine which of the reactions in exercise 5 is not a redox reaction explain your reasoning 2
Uploaded: 2020-10-18
Duration: 5 min 40 s
Channel: Numerade
Description: Determine which of the reactions in Exercise 5 is not a redox reaction. Explain your reasoning.

Question

Determine which of the reactions in Exercise 5 is not a redox reaction. Explain your reasoning.

Vishal Sharma · Accepted Answer

in problem six, which off? These in exercise five is not a redox reaction. So the occasion that is given in the exercise five days, zinc solid when rates with the Equus copper chloride. So it will form Cooper solid and a course zinc chloride. So this is the equation. This is the equation that is the that is in the party. So basically, this is the redox reaction. So this is the redox reaction, because we see that this think so. Zinc is converted into that NCL too. So that means it&#x27;s it can hear zinc does that into place so that we can see that this thing is converted into that in tow. Didn&#x27;t two plus I am. So basically, it&#x27;s lots of electrons, so we can say that it is the oxidation. So here, oxidation of using can take this and in case off reduction in case of reduction. So here. So this is the oxidation, and we can see that this copper chloride is converted into copper. So that means corporations converted into Cooper so ahead reduction can take place. So this is the reduction. So this is an example off redox reaction so sudden, solid plus copper chloride equals toe form. Cooper solid does. They didn&#x27;t sell toe questing chloride, of course. So it is a redox reaction. Redox reactions are those in which oxidation and reduction can take this simultaneously. Now, in the part B, when a quiz barium nitrate reacts with the Equis copper sell food, then it will form okay, Solid very himself with and a quest. Copper nitrate equals copper nitrate. No. So in this equation, we see that this very, um that in the left side off the equation that is in the plus to charge. And in the right hand side, it is again in the past to charge. So there is no change in its, uh, charge. Or we can say that it&#x27;s oxidation state and in case off copper, copper in copper sulfate is plus two and incorporated it is again plus two so that when there is no change in charge, So there s so it is not an example off redox reaction. So this is not a redox reaction. This is not a redox reaction. That mean we can say that the reaction be is reaction be is not a redox reaction. Because because there is no loss or gain off electrons because there is no laws or gain off electrons. Okay, No, Philip Tom&#x27;s also the oxidation state, So oxidation state is the charge. The same often element, according to some set off rule, is not change. Oxidation state quoth element is not change. So this is not other dogs. Direction. The logs reaction. See sulfate and nitrate, and that is again. It&#x27;s same oxidation state. So there is no change in oxidation state. Or we can say that there is no loss or gain off. Electron can take place in the equation. Be so this is not a redox reaction. So the reaction is, Ah, Redox reaction and the reaction B is not a Redox reaction.

Stephen Pulliam · Answer

in this question, you&#x27;re given two different equations and asked which of these is a Redox reaction? And so the best way to go about doing this is to assign oxidation numbers to everything to see what changes. And so you can see that lithium on the left is plus one, uh, oxygen on the left is minus two. Hydrogen on the left is plus one, and nitrogen is plus five. And that&#x27;s the same as what they are on the right side. So the top reaction there is not a Redox reaction. We&#x27;ll now turn our attention to the second reaction. The blue one down there. Ah, the I died is minus one, and magnesium is plus two and bro mean zero. It&#x27;s on the right side. You can see that the oxidation numbers for bro mean and iodine have changed. So therefore this bottom on the blue and is a redox reaction because there has been a change in the oxidation states of two of those elements in the reaction

Matthew Lueckheide · Answer

So you&#x27;re given to half reactions. You have to determine. Essentially determine which one is the oxidation. Have reaction. Which one is the reduction? Half reaction. A sign of reaction to the electrodes in ah, typical electrochemical cell. And then write the overall Redox reaction. So in these equations in these half reactions, when you&#x27;re electrons are products Um, this is gonna be the oxidation reaction because you&#x27;re cadmium metal starts is cadmium zero, and it&#x27;s losing two electrons. Um, the opposite of that silver plus plus one electron goes to silver zero. So that means that your silver is being reduced. Your oxidation state goes from positive +120 So the way that you assigned these to the electrodes is that oxidation happens that you&#x27;re an ode, the more, um more reactive metal. And then reduction happens at your cathode, so you&#x27;d have a silver cathode, a cadmium, an ode and in this particular cell, and then the way that you have to balance, you have to make an overall balance redox equation. So the way they do that is to make sure that you have the same amount of electrons on both sides, right? So you have to get the electrons in both half reactions to be equivalent in terms of the amount of electrons being transferred. So in this, in terms of ST geometry, I&#x27;m saying so. And so, cabbie, um, is transferring to electrons here. Um, but silver is only transferring one electron years. In order to balance the equation, we have to multiply this half reaction by two. So it&#x27;s gonna be two silver Adams. Um, well, each give or each taken electron, um, and that make two equivalents of silver zero. So you&#x27;ll see where this ties in when you read the overall half reaction. So now we multiply it by the, um, the reduction reaction by two. So ignore this right now, so we&#x27;re gonna add equation one here with Equation two here together to get the overall half reaction. So you&#x27;re gonna have cadmium solid. Plus two silver Adams. Um, plus two electrons is going to give you cadmium two plus plus two electrons plus two silver medal. Right. So you&#x27;ll see that the reason why we had to multiply that reduction reaction by too well so that our electrons will cancel out here. So if you&#x27;re in electrons, don&#x27;t cancel out when you go to make your balance Redox equation. You have to go back to the half reactions and multiply the whole thing by some coefficient to get the electrons to cancel out. When you add the an ode on the cathode half reactions together is your overall, um, equation is going to be cadmium solid. Plus two Silver plus is going to give you cadmium two plus plus two silver zero.

David Collins · Answer

Redox Reactions air fairly easy to identify If you know how to assign oxidation states. A Redox reaction is essentially identified by looking for a reactant element involved in a compound that has a change in its oxidation state. If you can identify any element with the change in oxidation states than it is a Redox reaction.

David Collins · Answer

to identify a reaction as a redox reaction, we must first assign oxidation states to all of the elements. If there&#x27;s a change in oxidation states going from the reactant to the products, then it&#x27;s a redox reaction. Otherwise, it&#x27;s not a redox reaction, aluminum all by itself has an oxidation state of zero. But when it becomes a three plus charge, it has an oxidation state of plus three. Silver with a plus one charge has an oxidation state of plus one all by itself. As an atom has an oxidation state of zero. So there&#x27;s a change in oxidation states. So this is a redox reaction. Aluminum has an increase in oxidation states. So it was oxidized, serving as the reducing agent. Silver has a decrease in oxidation states. So it was reduced serving as the oxidizing agent. The next reaction, when we assign oxidation states, we see that oxygen stays is minus two, hydrogen stays is plus one and sulfur stays is plus six. So this is not a redox reaction. Next, we have barium reacting with chlorine to produce barium chloride. Barium all by itself has an oxidation state of zero as barium chloride because its charges to plus it has an oxidation state of plus two Chlorine goes from zero to an oxidation state of -1. So there&#x27;s definitely changes in oxidation states. This is a redox reaction. Barium shows an increase in its oxidation state. So it was oxidized, thus serving as the reducing agent chlorine shows a decrease in its oxidation state. So it was reduced, serving as the oxidizing agent. Next we have magnesium reacting with roaming to produce magnesium bromide. Magnesium all by itself has an oxidation state of zero. Magnesium, with a Plus two or two plus charge has an oxidation state of plus two room. You know by itself, has an oxidation state of zero, but in the ionic compound, magnesium bromide with a one minus charge, it has a -1 Oxidation State. So there&#x27;s a change in oxidation states. This is a redox reaction. Magnesium shows an increase in oxidation states, so it was oxidized serving as the reducing agent. Roaming shows a decrease in oxidation states, so it was reduced serving as the oxidizing agent.

David Collins · Answer

to identify a reaction as a redox reaction, we need to see a change in oxidation states. So if it&#x27;s not a common reaction that we&#x27;ve already been introduced to, such as an acid base reaction or a precipitation reaction, we need to assign oxidation states to see if they change this reaction is lithium reacting with oxygen producing lithium oxide. The oxidation state of lithium by itself is zero. Oxygen is elemental oxygen is zero. lithium becomes plus one because that&#x27;s a new charge and oxygen becomes minus two. There&#x27;s definitely a change in oxidation states, lithium increases so it was oxidized and serves as the reducing agent. Oxygen has a decrease in its oxidation state. So it was reduced and serves as the oxidizing agent. For the next one, we have magnesium reacting with FP two plus producing mg two plus plus iron Magnesium by itself has an oxidation state of zero. It becomes plus two FB two plus has an oxidation state of plus two, it becomes zero. So magnesium shows an increase in its oxidation state. It was oxidized. So it serves as the reducing agent, An F two plus has decreased in its oxidation state. So it was reduced, serving as the oxidizing agent. The next two reactions are not redox reactions. Hopefully you recognize, see forms a solid precipitate. So this is a precipitation reaction and the last reaction is a strong acid hbR reacting with a strong base K. O. H. So it is an acid base reaction. There&#x27;s no change in oxidation states

Problem

Which of these reactions from Unit 4: Toxins can …

Problem 6 Easy Difficulty

Determine which of the reactions in Exercise 5 is not a redox reaction. Explain your reasoning.

Answer

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