Ch.20 - Electrochemistry

Problem 113e

Chapter 20, Problem 113e

Aqueous solutions of ammonia 1NH32 and bleach (active ingredient NaOCl) are sold as cleaning fluids, but bottles of both of them warn: 'Never mix ammonia and bleach, as toxic gases may be produced.' One of the toxic gases that can be produced is chloroamine, NH2Cl. (e) Is N oxidized, reduced, or neither, upon the conversion of ammonia to nitrogen trichloride?

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Identify the oxidation state of nitrogen in ammonia (NH_3).

Determine the oxidation state of nitrogen in nitrogen trichloride (NCl_3).

Compare the oxidation states of nitrogen in NH_3 and NCl_3.

If the oxidation state of nitrogen increases, it is oxidized; if it decreases, it is reduced; if it remains the same, it is neither.

Conclude whether nitrogen is oxidized, reduced, or neither based on the change in oxidation state.

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Key Concepts

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

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. Understanding these concepts is crucial for determining the changes in oxidation states of elements during chemical reactions.

Oxidation States

Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate their degree of oxidation or reduction. The oxidation state of an element in a compound can help track electron transfer during reactions. For example, in the conversion of ammonia to nitrogen trichloride, analyzing the oxidation states of nitrogen can reveal whether it is oxidized or reduced.

Chloroamines Formation

Chloroamines are a class of compounds formed when ammonia reacts with chlorine-containing agents, such as bleach. The formation of chloroamines involves the substitution of hydrogen atoms in ammonia with chlorine atoms, which can lead to the release of toxic gases. Understanding the chemistry of chloroamines is essential for assessing the safety and risks associated with mixing ammonia and bleach.

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Related Practice

Textbook Question

The Haber process is the principal industrial route for converting nitrogen into ammonia: N₂(g) + 3 H₂(g) → 2 NH₃(g) (b) Using the thermodynamic data in Appendix C, calculate the equilibrium constant for the process at room temperature.

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Open Question

In a galvanic cell, the cathode is an Ag+ | 1.00 M | Ag(s) half-cell. The anode is a standard hydrogen electrode immersed in a buffer solution containing 0.10 M benzoic acid (C6H5COOH) and 0.050 M sodium benzoate (C6H5COO-Na+). The measured cell voltage is 1.030 V. What is the pKa of benzoic acid?

Textbook Question

Aqueous solutions of ammonia 1NH32 and bleach (active ingredient NaOCl) are sold as cleaning fluids, but bottles of both of them warn: 'Never mix ammonia and bleach, as toxic gases may be produced.' One of the toxic gases that can be produced is chloroamine, NH2Cl. (b) What is the oxidation number of chlorine in chloramine?

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Open Question

A voltaic cell is based on Ag+ (aq) > Ag (s) and Fe3+ (aq) > Fe2+ (aq) half-cells. Use S° values in Appendix C and the relationship between cell potential and free-energy change to predict whether the standard cell potential increases or decreases when the temperature is raised above 25 °C.

Open Question

Hydrogen gas has the potential for use as a clean fuel in reaction with oxygen. The relevant reaction is 2 H2(g) + O2(g) → 2 H2O(l). Consider two possible ways of utilizing this reaction as an electrical energy source: (i) Hydrogen and oxygen gases are combusted and used to drive a generator, much as coal is currently used in the electric power industry; (ii) hydrogen and oxygen gases are used to generate electricity directly by using fuel cells that operate at 85 °C. Based on the analysis here, would it be more efficient to use the combustion method or the fuel-cell method to generate electrical energy from hydrogen?

Textbook Question

Cytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe to supply energy required to synthesize adenosine triphosphate (ATP). The body uses ATP as an energy source to drive other reactions (Section 19.7). At pH 7.0 the following reduction potentials pertain to this oxidation of CyFe2+: O21g2 + 4 H+1aq2 + 4 e- ¡ 2 H2O1l2 Ered ° = +0.82 V CyFe3+1aq2 + e- ¡ CyFe2+1aq2 E°red = +0.22 V (a) What is ∆G for the oxidation of CyFe2+ by air? (b) If the synthesis of 1.00 mol of ATP from adenosine diphosphate (ADP) requires a ∆G of 37.7 kJ, how many moles of ATP are synthesized per mole of O2?

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