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Chapter 9: Q18 E (page 508)

Sometimes leaving a bicycle in the sun on a hot day will cause a blowout. Why?

Short Answer

Expert verified

Sometimes leaving a bicycle in the sun on a hot day will cause a blowout, because the pressure is increased too much, and a tire will blow.

Step by step solution

01

Definition of Amonton's law

Guillaume Edmonton, a French physicist, discovered Amonton's law in the late 1600s. If the volume of a gas remains constant, Amonton's law states that increasing the temperature of the gas raises its pressure.

02

Explaining

The ideal gas law, or Amonton's law, states that the ratio of pressure to temperature remains constant at constant volume and quantity of gas particles. This indicates that if the volume and amount remain constant, a change in temperature will result in a change in pressure.

The air in bicycle tires is constantly warmed up by the sun on a sunny day. As a result, the temperature rises, and the pressure rises as well, according to Edmonton's law. Of course, we might suppose that the volume of tires and the number of molecules are both constant.

A tire will explode if the pressure is increased too much, resulting in a blowout on a sunny day.

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Most popular questions from this chapter

Question: When two cotton plugs, one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white ring of \({\rm{N}}{{\rm{H}}_{\rm{4}}}{\rm{Cl}}\) forms where gaseous \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) and gaseous \({\rm{HCl}}\) first come into contact. (Hint: Calculate the rates of diffusion for both \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) and \({\rm{HCl}}\), and find out how much faster \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) diffuses than \({\rm{HCl}}\).) \({\rm{N}}{{\rm{H}}_{\rm{3}}}{\rm{(g) + HCl(g)}} \to {\rm{N}}{{\rm{H}}_{\rm{4}}}{\rm{Cl(s)}}\)

At approximately what distance from the ammonia moistened plug does this occur?

Consider this scenario and answer the following questions: On a mid-August day in the north-eastern United States, the following information appeared in the local newspaper: atmospheric pressure at sea level 29.97 in. Hg,1013.9 mbar. (a) What was the pressure in kPa? (b) The pressure near the seacoast in the north-eastern United States is usually reported near 30.0 in. During a hurricane, the pressure may fall to near 28.0 in. Calculate the drop in pressure in torr.

A cylinder of medical oxygen has a volume of \({\rm{35}}{\rm{.4\;L}}\) and contains \({{\rm{O}}_{\rm{2}}}\)at a pressure of \({\rm{151 atm}}\) and a temperature of \({\rm{2}}{{\rm{5}}^{\rm{^\circ }}}{\rm{C}}\). What volume of \({{\rm{O}}_{\rm{2}}}\) does this correspond to at normal body conditions, that is, \({\rm{1 atm}}\)and\({\rm{3}}{{\rm{7}}^{\rm{^\circ }}}{\rm{C}}\)?

A \({\rm{20}}{\rm{.0 - L}}\) cylinder containing \({\rm{11}}{\rm{.34\;kg}}\)of butane, \({{\rm{C}}_{\rm{4}}}{{\rm{H}}_{{\rm{10}}}}\), is opened to the atmosphere. Calculate the mass of the gas remaining in the cylinder if the gas escapes until the pressure in the cylinder is equal to the atmospheric pressure, \({\rm{0}}{\rm{.983}}\)atm,ata temperature of \({\rm{2}}{{\rm{7}}^{\rm{^\circ }}}{\rm{C}}{\rm{.}}\)

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