Consider the following unbalanced oxidation-reduction reactions in aqueous solution: Ag + (aq) + Li(s) → Ag(s) + Li + (aq) Fe(s) + Na + (aq) → Fe 2+ (aq) + Na(s) K(s) + H 2 O(l) → KOH(aq) + H 2 (g) (d) Use the activity series to predict which of these reactions should occur. (Section 4.4) Are these results in accord with your conclusion in part (c) of this problem?

Hey, y'all. Let's get started on this next question. So based on the activity series, trends for the following halogen, predict the products for the following reactions. If no reaction occurs, right? No reaction. So let's actually see exactly what we're working with. We have a flooring Plus two sodium chloride yield to sodium fluoride, plus chlorine. Then we have chlorine plus two sodium bromide yields to sodium chloride and then um browning. So as we can see, we have halogen is here. So we have flooring and chlorine and we also have chlorine and brewing. And so essentially what's happening is we have our reactivity um series. So let's look at our halogen. So we're looking at group seven a and essentially the way that the reactivity works is we have Florence, the most reactive than chlorine, then bruning then iodine. And so reactivity goes up as you move up. So reactivity increases. Now here's the thing um a more reactive atom or element can displace a less reactive element, but a less reactive element cannot displace a more reactive one. So here what's happening for this equation or this reaction? The more reactive flooring is displacing the chlorine. So that's why we're getting the sodium fluoride and then here the more reactive chlorine is displacing the broad means. So we're getting our sodium chloride. So let's look at number one. We want to predict the products right here. So chlorine plus lithium floor ideals. What now here, what we would see is we would see a reaction um that would form lithium chloride Plus flooring. However, that cannot occur here. So this is going to be no reaction. The reason being is because chlorine cannot displace an already reactive flooring because chlorine is higher up on this list. Let's move on to the next one. So let me highlight. That's the answer here for the next one. We have chlorine plus magnesium bromide. Now because the chlorine is higher up than bruning, we know that chlorine will be able to displace the bruning. And so what we're going to have is we're going to have magnesium chloride plus roaming So these are going to be your products. So these are going to be your final answers. Alright, everyone. I really hope this video helped and I will see you in the next one.

Ch.5 - Thermochemistry

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Brown 14th Edition

Ch.5 - Thermochemistry

Problem 121d

Chapter 5, Problem 121d

Consider the following unbalanced oxidation-reduction reactions in aqueous solution:
Ag⁺(aq) + Li(s) → Ag(s) + Li⁺(aq)
Fe(s) + Na⁺(aq) → Fe²⁺(aq) + Na(s)
K(s) + H₂O(l) → KOH(aq) + H₂(g)
(d) Use the activity series to predict which of these reactions should occur. (Section 4.4) Are these results in accord with your conclusion in part (c) of this problem?

Verified step by step guidance

Identify the activity series of metals, which ranks metals by their ability to displace other metals from solutions of their ions. Metals higher in the series can displace metals lower in the series from their compounds.

For the reaction Ag+(aq) + Li(s) → Ag(s) + Li+(aq), compare the positions of Li and Ag in the activity series. Lithium is higher than silver, indicating that lithium can displace silver ions from solution, making this reaction feasible.

For the reaction Fe(s) + Na+(aq) → Fe2+(aq) + Na(s), compare the positions of Fe and Na in the activity series. Sodium is higher than iron, suggesting that iron cannot displace sodium ions from solution, making this reaction not feasible.

For the reaction K(s) + H2O(l) → KOH(aq) + H2(g), check the activity series to see if potassium can react with water. Potassium is highly reactive and can displace hydrogen from water, making this reaction feasible.

Summarize the findings: The reactions that should occur based on the activity series are the first and third reactions. The second reaction should not occur. Compare these predictions with the conclusions from part (c) to see if they align.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the reactants and products is crucial for predicting the feasibility of the reactions presented.

Activity Series

The activity series is a list of metals ranked by their ability to displace other metals from compounds in solution. A more reactive metal can displace a less reactive metal from its compound, which helps predict whether a reaction will occur. In the context of the given reactions, comparing the metals involved with their positions in the activity series will determine if the reactions are feasible.

Aqueous Solutions and Solubility

Aqueous solutions involve substances dissolved in water, where solubility plays a key role in determining whether a reaction can occur. Some products of reactions may precipitate out of solution, while others remain dissolved. Understanding the solubility rules and the behavior of ions in solution is essential for analyzing the outcomes of the reactions presented in the question.

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Related Practice

Textbook Question

Suppose an Olympic diver who weighs 52.0 kg executes a straight dive from a 10-m platform. At the apex of the dive, the diver is 10.8 m above the surface of the water. (b) Assuming that all the potential energy of the diver is converted into kinetic energy at the surface of the water, at what speed, in m/s, will the diver enter the water?

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Textbook Question

Consider the following unbalanced oxidation-reduction reactions in aqueous solution:

Ag⁺(aq) + Li(s) → Ag(s) + Li⁺(aq)

Fe(s) + Na⁺(aq) → Fe²⁺(aq) + Na(s)

K(s) + H₂O(l) → KOH(aq) + H₂(g)

(a) Balance second reaction.

681

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Textbook Question

Consider the following unbalanced oxidation-reduction reactions in aqueous solution:

Ag⁺(aq) + Li(s) → Ag(s) + Li⁺(aq)

Fe(s) + Na⁺(aq) → Fe²⁺(aq) + Na(s)

K(s) + H₂O(l) → KOH(aq) + H₂(g)

(a) Balance third reaction.

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Textbook Question

Consider the following acid-neutralization reactions involvingthe strong base NaOH(aq):HNO31aq2 + NaOH1aq2¡NaNO31aq2 + H2O1l2HCl1aq2 + NaOH1aq2¡NaCl1aq2 + H2O1l2NH4+1aq2 + NaOH1aq2¡NH31aq2 + Na+1aq2 + H2O1l2(d) In the third equation NH4+1aq2 is acting as an acid. Basedon the value of H° for this reaction, do you think it is astrong or a weak acid? Explain.

Consider two solutions, the first being 50.0 mL of 1.00 M CuSO₄ and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 to 27.7 °C (d) From the calorimetric data, calculate ΔH for the reaction that occurs on mixing. Assume that the calorimeter absorbs only a negligible quantity of heat, that the total volume of the solution is 100.0 mL, and that the specific heat and density of the solution after mixing are the same as those of pure water.