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Chapter 16: Q16.1-5E (page 906)

Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to form carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.

Short Answer

Expert verified

Plastics are kinetically stable and do not decompose rapidly even over long periods of time.

Step by step solution

01

Definition of Spontaneous reaction.

  • The term "spontaneous reaction" refers to a reaction that does not involve the application of any external force or energy. Lied to a forward reaction by using non-spontaneous reactions.
02

Determine that plastics are tend to persist in the environment.

  • The rate of oxidation tends to be very slow even when the oxidation of plastics happens spontaneously.
  • In order to go forward, they require external energy. Organic polymers are used to make plastics.
  • Carbon and hydrogen make up their structure. When they come into contact with oxygen in the air, they produce carbon dioxide and water. This is the result of oxidation on plastic.
  • Although it is a spontaneous reaction, the oxidation is gradual and the decomposition takes a long time.
  • Plastic materials, as a result, tend to persist in the environment on our kinetically stable.

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Most popular questions from this chapter

Use the thermodynamic data provided in Appendix G to calculate the equilibrium constant for the dissociation of dinitrogen tetraoxide at 25 °C.

Balance the following reactions and write the reactions using cell notation. Ignore any inert electrodes, as they are never part of the half-reactions.

(a) \({\rm{Al}}(s) + {\rm{Z}}{{\rm{r}}^{4 + }}(aq) \to {\rm{A}}{{\rm{l}}^{3 + }}(aq) + {\rm{Zr}}(s)\)

(b) \({\rm{A}}{{\rm{g}}^ + }(aq) + {\rm{NO}}(g) \to {\rm{Ag}}(s) + {\rm{N}}{{\rm{O}}_3}^ - (aq)\)(acidic solution)

(c) \({\rm{Si}}{{\rm{O}}_3}^{2 - }(aq) + {\rm{Mg}}(s) \to {\rm{Si}}(s) + {\rm{Mg}}{({\rm{OH}})_2}(s)\)(basic solution)

(d) \({\rm{Cl}}{{\rm{O}}_3}^ - (aq) + {\rm{Mn}}{{\rm{O}}_2}(s) \to {\rm{C}}{{\rm{l}}^ - }(aq) + {\rm{Mn}}{{\rm{O}}_4}^ - (aq)\)(basic solution

What is a spontaneous reaction?

Among other things, an ideal fuel for the control thrusters of a space vehicle should decompose in a spontaneous exothermic reaction when exposed to the appropriate catalyst. Evaluate the following substances under standard state conditions as suitable candidates for fuels.

(a) Ammonia\({\bf{:}}{\rm{ }}{\bf{2N}}{{\bf{H}}_{\bf{3}}}{\bf{(g)}} \to {{\bf{N}}_{\bf{2}}}{\bf{(g) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g)}}\)

(b) Diborane\({\bf{:}}{\rm{ }}{{\bf{B}}_{\bf{2}}}{{\bf{H}}_{\bf{6}}}{\bf{(g)}} \to {\bf{2\;B(g) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g)}}\)

(c) Hydrazine: \({{\bf{N}}_{\bf{2}}}{{\bf{H}}_{\bf{4}}}{\bf{(g)}} \to {{\bf{N}}_{\bf{2}}}{\bf{(g) + 2}}{{\bf{H}}_{\bf{2}}}{\bf{(g)}}\)

(d) Hydrogen peroxide: \({{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(l)}} \to {{\bf{H}}_{\bf{2}}}{\bf{O(g) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

Calculate the standard entropy change for the following reaction:

\({\bf{Ca(OH}}{{\bf{)}}_{\bf{2}}}{\bf{(\;s)}} \to {\bf{CaO(s) + }}{{\bf{H}}_{\bf{2}}}{\bf{O(l)}}\)
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