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Chapter 18: Problem 34

(a) With respect to absorption of radiant energy, what distinguishes a greenhouse gas from a nongreenhouse gas? (b) \(\mathrm{CH}_{4}\) is a greenhouse gas, but \(\mathrm{N}_{2}\) is not. How might the molecular structure of \(\mathrm{CH}_{4}\) explain why it is a greenhouse gas?

Short Answer

Expert verified
(a) Greenhouse gases can effectively absorb and emit infrared radiation due to their molecular structure, which allows them to vibrate in ways that can absorb the energy of infrared radiation. Non-greenhouse gases do not absorb or emit infrared radiation effectively due to their limited vibrational modes. (b) The tetrahedral molecular structure of methane (\(\mathrm{CH}_{4}\)) enables a variety of vibrational modes that match the energies of infrared radiation, making it a greenhouse gas. In contrast, the linear and symmetric structure of nitrogen (\(\mathrm{N}_{2}\)) limits its capacity for vibrations that can absorb infrared radiation, making it a non-greenhouse gas.

Step by step solution

01

Define Greenhouse Gas and Non-Greenhouse Gas

Greenhouse gases are those gases in the Earth's atmosphere that can absorb and emit infrared radiation, thus, trapping and holding heat. Non-greenhouse gases do not effectively absorb or emit infrared radiation, thus, they do not play a significant role in the trapping and holding of heat.
02

Discuss the reason behind absorption of radiant energy by greenhouse gases.

Greenhouse gases can effectively absorb and emit infrared radiation due to their molecular structure that allows them to vibrate in a way that can absorb the energy of infrared radiation. These vibrations can occur in multiple ways, such as stretching or bending of bonds between the atoms within the molecule.
03

Examine the molecular structure of CH4 (methane).

Methane (CH4) is a tetrahedral molecule with one carbon atom at the center and four hydrogen atoms surrounding it. The bonds between the carbon and hydrogen atoms can vibrate in various modes, like the symmetric stretch, the asymmetric stretch, and bending vibrations. These vibrations enable methane to effectively absorb and emit infrared radiation.
04

Examine the molecular structure of N2 (nitrogen).

Nitrogen (N2) is a diatomic molecule, consisting of two nitrogen atoms bonded together by a triple bond. Due to its linear and symmetric structure, nitrogen has very limited ways of vibrating, which are not compatible with the absorption of infrared radiation.
05

Relate the molecular structures to their greenhouse properties.

The molecular structure of CH4 allows it to have a variety of vibrational modes that match the energies of infrared radiation, making it an effective greenhouse gas. In contrast, the linear and symmetric structure of N2 limits its capacity for vibrations that can absorb infrared radiation, making it a non-greenhouse gas. In conclusion, the molecular structure plays a significant role in determining whether a gas can effectively absorb and emit infrared radiation, classifying it as a greenhouse gas or a non-greenhouse gas. Methane's tetrahedral structure enables it to absorb infrared radiation, while nitrogen's diatomic structure does not.

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Most popular questions from this chapter

One of the possible consequences of climate change is an increase in the temperature of ocean water. The oceans serve as a "sink" for \(\mathrm{CO}_{2}\) by dissolving large amounts of it. (a) How would the solubility of \(\mathrm{CO}_{2}\) in the oceans be affected by an increase in the temperature of the water? (b) Discuss the implications of your answer to part (a) for the problem of climate change.

(a) Explain why \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitates when \(\mathrm{CO}_{3}^{2-}\) ion is added to a solution containing \(\mathrm{Mg}^{2+}\). . (b) Will \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitate when \(4.0 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is added to \(1.00 \mathrm{~L}\) of a solution containing 125 ppm of \(\mathrm{Mg}^{2+}\) ?

The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. (a) Using the density, specific heat, and heat of vaporization of water from Appendix \(\mathrm{B}\), calculate the amount of energy required to vaporize 1.00 gal of water beginning with water at \(20^{\circ} \mathrm{C}\). (b) If the energy is provided by electricity costing \(\$ 0.085 / \mathrm{kWh},\) calculate its cost. (c) If distilled water sells in a grocery store for \(\$ 1.26\) per gal, what percentage of the sales price is represented by the cost of the energy?

Describe the basic goals of green chemistry. [Section 18.5\(]\)

The following data were collected for the destruction of \(\mathrm{O}_{3}\) by \(\mathrm{H}\left(\mathrm{O}_{3}+\mathrm{H} \longrightarrow \mathrm{O}_{2}+\mathrm{OH}\right)\) at very low concentrations: $$ \begin{array}{llll} \hline \text { Trial } & {\left[\mathrm{O}_{3}\right](\boldsymbol{M})} & {[\mathrm{H}](\boldsymbol{M})} & \text { Initial Rate }(\boldsymbol{M} / \mathrm{s}) \\ \hline 1 & 5.17 \times 10^{-33} & 3.22 \times 10^{-26} & 1.88 \times 10^{-14} \\\ 2 & 2.59 \times 10^{-33} & 3.25 \times 10^{-26} & 9.44 \times 10^{-15} \\ 3 & 5.19 \times 10^{-33} & 6.46 \times 10^{-26} & 3.77 \times 10^{-14} \\ \hline \end{array} $$ (a) Write the rate law for the reaction. (b) Calculate the rate constant.
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