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Chapter 18: Problem 29

Nitrogen oxides like \(\mathrm{NO}_{2}\) and \(\mathrm{NO}\) are a significant source of acid rain. For each of these molecules write an equation that shows how an acid is formed from the reaction with water.

Short Answer

Expert verified
The balanced chemical equations for the formation of acids from nitrogen oxides reacting with water are: 1. For NO鈧�: \(NO鈧� (g) + H鈧侽 (l) \rightarrow HNO鈧� (aq) + HNO鈧� (aq)\) 2. For NO: \(2NO (g) + 2H鈧侽 (l) \rightarrow 2HNO鈧� (aq) + NH鈧侽H (aq)\)

Step by step solution

01

Formation of nitric acid from NO鈧�

When nitrogen dioxide (NO鈧�) reacts with water, nitric acid (HNO鈧�) and nitrous acid (HNO鈧�) are formed as products. The balanced chemical equation for this reaction is: \(NO鈧� (g) + H鈧侽 (l) \rightarrow HNO鈧� (aq) + HNO鈧� (aq)\) Step 2: Write the equation for NO reacting with water.
02

Formation of nitrous acid from NO

When nitric oxide (NO) reacts with water, nitrous acid (HNO鈧�) and hydroxylamine (NH鈧侽H) are formed as products. The balanced chemical equation for this reaction is: \(2NO (g) + 2H鈧侽 (l) \rightarrow 2HNO鈧� (aq) + NH鈧侽H (aq)\) Now we have both reactions showing the formation of acids from nitrogen oxides reacting with water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Nitrogen Oxides
Nitrogen oxides are a group of gases that play a crucial role in environmental chemistry. These gases include primarily nitrogen dioxide \((\mathrm{NO}_2)\) and nitric oxide \((\mathrm{NO})\). Nitrogen oxides are introduced into the atmosphere through both natural processes, like lightning, and human activities, such as burning fossil fuels. Once in the atmosphere, they contribute to a range of environmental issues.

  • They are key precursors to acid rain.
  • Nitrogen oxides also have effects on respiratory health.
  • They participate in the formation of ozone at ground level.
Understanding the transformations of these compounds is essential for addressing their impact on the environment and public health.
Chemical Reactions
Chemical reactions are processes where substances are transformed into new products with different properties. In the context of nitrogen oxides, these reactions are critical for understanding how these compounds interact with other elements and compounds in the environment.
  • For example, nitrogen dioxide \((\mathrm{NO}_2)\) reacts with water to form acids.
  • The chemical equations involved are crucial for predicting the outcomes and impacts of these reactions.
These reactions are balanced, meaning the number of atoms for each element are conserved in the process. For nitrogen oxide reactions, this means careful consideration of reactants and products to ensure the chemical equations adhere to the Law of Conservation of Mass.
Nitric Acid Synthesis
Nitric acid \((\mathrm{HNO}_3)\) is a strong acid formed when nitrogen dioxide \((\mathrm{NO}_2)\) reacts with water. This reaction is an integral part of the process contributing to acid rain formation. The equation for this reaction is: \[\mathrm{NO}_2 (g) + \mathrm{H}_2\mathrm{O} (l) \rightarrow \mathrm{HNO}_3 (aq) + \mathrm{HNO}_2 (aq)\]This balanced chemical equation shows that both nitric acid and nitrous acid \((\mathrm{HNO}_2)\) are produced when \(\mathrm{NO}_2\) is dissolved in water.

  • Nitric acid formation is a major pathway for nitrogen oxides to contribute to acid rain.
  • The presence of nitric acid can lead to lowered pH levels in rainwater, adversely affecting ecosystems.
Nitrous Acid Formation
Nitrous acid \((\mathrm{HNO}_2)\) is another product formed in reactions of nitrogen oxides with water. In the case of nitric oxide \((\mathrm{NO})\), it reacts with water following this equation:\[2\mathrm{NO} (g) + 2\mathrm{H}_2\mathrm{O} (l) \rightarrow 2\mathrm{HNO}_2 (aq) + \mathrm{NH}_2\mathrm{OH} (aq)\]In addition to producing nitrous acid, hydroxylamine \((\mathrm{NH}_2\mathrm{OH})\) is also formed. These reactions highlight the transformative nature of chemical reactions involving nitrogen oxides.

  • Nitrous acid is a weaker acid than nitric acid but still contributes to environmental acidity.
  • This acid can further decompose and participate in various atmospheric chemical processes, influencing environmental conditions.
Understanding these reactions is important for comprehending how nitrogen oxides alter the chemistry of our atmosphere.

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Most popular questions from this chapter

You are working with an artist who has been commissioned to make a sculpture for a big city in the eastern United States. The artist is wondering what material to use to make her sculpture because she has heard that acid rain in the eastern United States might destroy it over time. You take samples of granite, marble, bronze, and other materials, and place them outdoors for a long time in the big city. You periodically examine the appearance and measure the mass of the samples. (a) What observations would lead you to conclude that one or more of the materials are wellsuited for the sculpture? (b) What chemical process (or processes) is (are) the most likely responsible for any observed changes in the materials? [Section 18.2\(]\)

In 2008 , the global average electricity consumption per head was \(3.0 \mathrm{MWh}\). The solar power striking Earth every day averages 168 watts per square meter. Considering that present technology for solar energy conversion is about \(10 \%\) efficient, from how many square meters of land must sunlight be collected in order to provide this power?

(a) It has been reported, that acid rain with a pH of 3.5 could corrode mild steel. Write a chemical equation that describes the attack of acid rain on an iron (Fe) material. (b) If the iron material were covered with a surface layer of copper, would this help to stop the effects of acid rain? Explain.

Draw the Lewis structure for the chlorofluorocarbon CFC-11, \(\mathrm{CFCl}_{3}\). What chemical characteristics of this substance allow it to effectively deplete stratospheric ozone?

Although there are many ions in seawater, the overall charges of the dissolved cations and anions must maintain charge neutrality. Consider only the six most abundant ions in seawater, as listed in Table \(18.5\left(\mathrm{Cl}^{-}, \mathrm{Na}^{+},\right.\) \(\mathrm{SO}_{4}^{2-}, \mathrm{Mg}^{2+}, \mathrm{Ca}^{2+},\) and \(\left.\mathrm{K}^{+}\right),\) calculate the total charge in Coulombs of the cations in \(1.0 \mathrm{~L}\) of seawater. Calculate the total charge in Coulombs of the anions in \(1.0 \mathrm{~L}\) of seawater. To how many significant figures are the two numbers equal?
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