Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 43

In aqueous solution, hydrogen sulfide reduces (a) \(\mathrm{Fe}^{3+}\) to \(\mathrm{Fe}^{2+},(\mathbf{b}) \mathrm{Br}_{2}\) to \(\mathrm{Br}^{-},(\mathbf{c}) \mathrm{MnO}_{4}^{-}\) to \(\mathrm{Mn}^{2+},(\mathbf{d}) \mathrm{HNO}_{3}\) to \(\mathrm{NO}_{2}\) In all cases, under appropriate conditions, the product is elemental sulfur. Write a balanced net ionic equation for each reaction.

Short Answer

Expert verified
The balanced net ionic equations for the given reactions are: Case (a): \(2 \, H_2S + 4Fe^{3+} \rightarrow S_2 + 4H^+ + 4Fe^{2+}\) Case (b): \(2 \, H_2S + Br_2 \rightarrow S_2 + 4H^+ + 4Br^-\) Case (c): \(5 \, H_2S + 4MnO_4^- + 16H^+ \rightarrow 2S_2 + 20H^+ + 4Mn^{2+} + 8H_2O\) Case (d): \(2 \, H_2S + 2HNO_3 \rightarrow S_2 + 4H^+ + 2NO_2 + 2H_2O\)

Step by step solution

01

Case (a): Fe³⁺ to Fe²⁺

For this reaction, we will write the oxidation half-reaction of hydrogen sulfide and the reduction half-reaction of Fe³⁺. Oxidation half-reaction: \(2 \, H_2S \rightarrow S_2 + 4H^+ + 4e^-\) Reduction half-reaction: \(Fe^{3+} + e^- \rightarrow Fe^{2+}\) To balance the charges and electrons, we need to multiply the reduction half-reaction by 4. This allows us to combine the two half-reactions to create the balanced net ionic equation: Final balanced net ionic equation: \(2 \, H_2S + 4Fe^{3+} \rightarrow S_2 + 4H^+ + 4Fe^{2+}\)
02

Case (b): Br₂ to Br⁻

For this case, we will write the oxidation half-reaction of hydrogen sulfide and the reduction half-reaction of Br₂. Oxidation half-reaction: \(2 \, H_2S \rightarrow S_2 + 4H^+ + 4e^-\) Reduction half-reaction: \(Br_2 + 2e^- \rightarrow 2Br^-\) To balance the charges and electrons, we need to multiply the reduction half-reaction by 2. This allows us to combine the two half-reactions to create the balanced net ionic equation: Final balanced net ionic equation: \(2 \, H_2S + Br_2 \rightarrow S_2 + 4H^+ + 4Br^-\)
03

Case (c): MnO₄⁻ to Mn²⁺

For this case, we will write the oxidation half-reaction of hydrogen sulfide and the reduction half-reaction of MnO₄⁻. Oxidation half-reaction: \(2 \, H_2S \rightarrow S_2 + 4H^+ + 4e^-\) Reduction half-reaction: \(MnO_4^- + 8H^+ + 5e^- \rightarrow Mn^{2+} + 4H_2O\) To balance the charges and electrons, we need to multiply the oxidation half-reaction by 5/2 and the reduction half-reaction by 2. This allows us to combine the two half-reactions to create the balanced net ionic equation: Final balanced net ionic equation: \(5 \, H_2S + 4MnO_4^- + 16H^+ \rightarrow 2S_2 + 20H^+ + 4Mn^{2+} + 8H_2O\)
04

Case (d): HNO₃ to NO₂

For this case, we will write the oxidation half-reaction of hydrogen sulfide and the reduction half-reaction of HNO₃. Oxidation half-reaction: \(2 \, H_2S \rightarrow S_2 + 4H^+ + 4e^-\) Reduction half-reaction: \(2HNO_3 + 2e^- \rightarrow 2NO_2 + 2H_2O\) We can simply combine the two half-reactions to create the balanced net ionic equation: Final balanced net ionic equation: \(2 \, H_2S + 2HNO_3 \rightarrow S_2 + 4H^+ + 2NO_2 + 2H_2O\)

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Both dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\), and methylhydrazine, \(\mathrm{CH}_{3} \mathrm{NHNH}_{2}\), have been used as rocket fuels. When dinitrogen tetroxide $\left(\mathrm{N}_{2} \mathrm{O}_{4}\right)$ is used as the oxidizer, the products are \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CO}_{2}\), and \(\mathrm{N}_{2}\). If the thrust of the rocket depends on the volume of the products produced, which of the substituted hydrazines produces a greater thrust per gram total mass of oxidizer plus fuel? (Assume that both fuels generate the same temperature and that \(\mathrm{H}_{2} \mathrm{O}(g)\) is formed.)

Write a balanced equation for each of the following reactions: (a) Burning magnesium metal in a carbon dioxide atmosphere reduces the \(\mathrm{CO}_{2}\) to carbon. (b) \(\mathrm{In}\) photosynthesis, solar energy is used to produce glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) and \(\mathrm{O}_{2}\) from carbon dioxide and water. (c) When carbonate salts dissolve in water, they produce basic solutions.

The \(\mathrm{SF}_{5}^{-}\) ion is formed when \(\mathrm{SF}_{4}(g)\) reacts with fluoride salts containing large cations, such as \(\mathrm{CsF}(s)\). Draw the Lewis structures for \(\mathrm{SF}_{4}\) and \(\mathrm{SF}_{5}^{-}\), and predict the molecular structure of each.

Manganese silicide has the empirical formula \(\mathrm{MnSi}\) and melts at \(1280^{\circ} \mathrm{C}\). It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect \(\mathrm{MnSi}\) to be: metallic, molecular, covalent-network, or ionic? (b) Write a likely balanced chemical equation for the reaction of MnSi with concentrated aqueous \(\mathrm{HF}\).

Consider the elements \(\mathrm{N}, \mathrm{F}, \mathrm{Si}, \mathrm{Rb},\) Te, and Ir. From this list, select the element that \((\mathbf{a})\) is most electronegative, \((\mathbf{b})\) exhibits a maximum oxidation state of \(+6,(\mathbf{c})\) loses an electron most readily, (d) forms \(\pi\) bonds most readily, (e) is a transition metal, \((\mathbf{f})\) forms four covalent bonds to achieve octet.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free