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Chapter 18: Problem 120

Comment on whether \(\mathrm{F}_{2}\) will become a stronger oxidizing agent with increasing \(\mathrm{H}^{+}\) concentration.

Short Answer

Expert verified
According to the provided information, increasing the \( \mathrm{H}^{+} \) concentration will not make \(\mathrm{F}_{2}\) a stronger oxidizing agent.

Step by step solution

01

Understand the relevant reaction

Consider the following half-reaction: \(\mathrm{F}_{2} + 2e^- \rightarrow 2\mathrm{F}^{-}\). Here, Fluorine is acting as an oxidizing agent because it is accepting electrons.
02

Determine the effect of \( \mathrm{H}^{+} \) ions

In this reaction, the concentration of \( \mathrm{H}^{+} \) ions does not have a direct role. Therefore, changing this concentration will not directly influence the ability of Fluorine to act as an oxidizing agent.
03

Reason from the perspective of Le Chatelier's principle

However, if other reactions are involved where \( \mathrm{H}^{+} \) ions are implicated, the situation might change according to Le Chatelier’s principle (which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change). For this specific query though, since no such other reactions are mentioned, it can be concluded as per the given information that an increase in \( \mathrm{H}^{+} \) concentration will not make \(\mathrm{F}_{2}\) a stronger oxidizing agent.

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Most popular questions from this chapter

Calculate the standard emf of a cell that uses the \(\mathrm{Mg} / \mathrm{Mg}^{2+}\) and \(\mathrm{Cu} / \mathrm{Cu}^{2+}\) half-cell reactions at \(25^{\circ} \mathrm{C}\) Write the equation for the cell reaction that occurs under standard-state conditions.

The zinc-air battery shows much promise for electric cars because it is lightweight and rechargeable: The net transformation is \(\mathrm{Zn}(s)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnO}(s)\) (a) Write the half-reactions at the zinc-air electrodes and calculate the standard emf of the battery at \(25^{\circ} \mathrm{C}\). (b) Calculate the emf under actual operating conditions when the partial pressure of oxygen is 0.21 atm. (c) What is the energy density (measured as the energy in kilojoules that can be obtained from \(1 \mathrm{~kg}\) of the metal) of the zinc electrode? (d) If a current of \(2.1 \times 10^{5} \mathrm{~A}\) is to be drawn from a zinc-air battery system, what volume of air (in liters) would need to be supplied to the battery every second? Assume that the temperature is \(25^{\circ} \mathrm{C}\) and the partial pressure of oxygen is 0.21 atm.

Explain why most useful galvanic cells give voltages of no more than 1.5 to \(2.5 \mathrm{~V}\). What are the prospects for developing practical galvanic cells with voltages of \(5 \mathrm{~V}\) or more?

Fluorine \(\left(\mathrm{F}_{2}\right)\) is obtained by the electrolysis of liquid hydrogen fluoride (HF) containing potassium fluoride (KF). (a) Write the half-cell reactions and the overall reaction for the process. (b) What is the purpose of KF? (c) Calculate the volume of \(\mathrm{F}_{2}\) (in liters) collected at \(24.0^{\circ} \mathrm{C}\) and 1.2 atm after electrolyzing the solution for \(15 \mathrm{~h}\) at a current of 502 A.

An aqueous KI solution to which a few drops of phenolphthalein have been added is electrolyzed using an apparatus like the one shown here: Describe what you would observe at the anode and the cathode. (Hint: Molecular iodine is only slightly soluble in water, but in the presence of \(\mathrm{I}^{-}\) ions, it forms the brown color of \(\mathrm{I}_{3}^{-}\) ions. See Problem \(12.102 .\)
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