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Chapter 5: Problem 1

Consider the following apparatus: a test tube covered with a nonpermeable elastic membrane inside a container that is closed with a cork. A syringe goes through the cork. a. As you push down on the syringe, how does the membrane covering the test tube change? b. You stop pushing the syringe but continue to hold it down. In a few seconds, what happens to the membrane?

Short Answer

Expert verified
a. As you push down on the syringe, the pressure inside the container increases, causing the elastic membrane to stretch and respond to the applied pressure. b. When you stop pushing the syringe but hold it down, the membrane tries to achieve equilibrium as the air pressure equalizes throughout the container. The membrane may show slight changes, such as relaxation or tension, depending on its elasticity, and will likely stay in place as long as the pressure is still higher on the outside than inside the test tube.

Step by step solution

01

Visualize the setup

Imagine a container with a cork, and a syringe going through the cork. Inside the container, there is a test tube covered by a nonpermeable elastic membrane.
02

Explain the effect of pushing down on the syringe

As you push down on the syringe, the pressure from air being compressed in the container increases. This increased pressure causes the elastic membrane to stretch and respond to the applied pressure. Part b:
03

Visualize the changed situation

You stop pushing the syringe but continue to hold it down. The air pressure remains high in the container as the air is trapped inside.
04

Explain the effect on the membrane

In a few seconds, the membrane would try to achieve equilibrium as the air pressure tries to equalize throughout the container. The membrane may show some slight changes, such as slight relaxation or tension, depending on how elastic and flexible it is. The membrane will likely stay in place as long as the pressure is still higher on the outside than inside the test tube.

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Most popular questions from this chapter

At \(0^{\circ} \mathrm{C}\) a \(1.0-\mathrm{L}\) flask contains \(5.0 \times 10^{-2} \mathrm{~mol} \mathrm{~N}_{2}, 1.5 \times 10^{2} \mathrm{mg}\) \(\mathrm{O}_{2}\), and \(5.0 \times 10^{21}\) molecules of \(\mathrm{NH}_{3} .\) What is the partial pressure of each gas, and what is the total pressure in the flask?

Sulfur trioxide, \(\mathrm{SO}_{3}\), is produced in enormous quantities each year for use in the synthesis of sulfuric acid. $$ \begin{aligned} \mathrm{S}(s)+\mathrm{O}_{2}(g) & \longrightarrow \mathrm{SO}_{2}(g) \\ 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{SO}_{3}(g) \end{aligned} $$ What volume of \(\mathrm{O}_{2}(g)\) at \(350 .{ }^{\circ} \mathrm{C}\) and a pressure of \(5.25 \mathrm{~atm}\) is needed to completely convert \(5.00 \mathrm{~g}\) sulfur to sulfur trioxide?

The partial pressure of \(\mathrm{CH}_{4}(g)\) is \(0.175\) atm and that of \(\mathrm{O}_{2}(g)\) is \(0.250\) atm in a mixture of the two gases. a. What is the mole fraction of each gas in the mixture? b. If the mixture occupies a volume of \(10.5 \mathrm{~L}\) at \(65^{\circ} \mathrm{C}\), calculate the total number of moles of gas in the mixture. c. Calculate the number of grams of each gas in the mixture.

Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions \(78 \% \mathrm{~N}_{2}, 21 \% \mathrm{O}_{2}\), and \(1.0 \% \mathrm{Ar}\), what is the density of air at standard temperature and pressure?

A spherical glass container of unknown volume contains helium gas at \(25^{\circ} \mathrm{C}\) and \(1.960 \mathrm{~atm}\). When a portion of the helium is withdrawn and adjusted to \(1.00\) atm at \(25^{\circ} \mathrm{C}\), it is found to have a volume of \(1.75 \mathrm{~cm}^{3}\). The gas remaining in the first container shows a pressure of \(1.710\) atm. Calculate the volume of the spherical container.
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