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Chapter 12: Problem 85

Explain why you feel resistance if you try to compress a sample of gas inside a plugged syringe.

Short Answer

Expert verified
Resistance is felt when compressing a gas in a plugged syringe because, according to the kinetic molecular theory, compressing the gas increases the number and frequency of particle collisions against the syringe wall. These collisions create a greater force per unit area, or pressure, resulting in the gas exerting a reaction force that is felt as resistance.

Step by step solution

01

Understanding the Composition of Gases

Gases are made up of small particles constantly in motion, which are relatively far apart compared to solids and liquids. These particles move in unpredictable, random straight paths and frequently collide with each other and the walls of their container, like the inside of the syringe.
02

Effect of Compression on Gas

When effort is made to compress a gas, i.e., decrease its volume, the particles are forced closer together. These particles still continue to move and collide but now over a much smaller volume, leading to a drastic increase in the number of collisions with each other and the syringe’s walls.
03

Concept of Pressure

Pressure is the force exerted by gas per unit area on the walls of its container. As the number of collisions increases on compression, the force exerted on the walls of the syringe also increases, thereby increasing the gas pressure inside the syringe.
04

Experiencing Resistance

The resistance felt when trying to compress the gas inside the syringe is the reaction force exerted by the gas due to this increase in pressure. According to Newton's third law, every action has an equal and opposite reaction. So when force is applied to compress the gas, the increased pressure causes the gas to exert an equal force in the opposite direction, which is felt as resistance.

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Most popular questions from this chapter

Suppose a certain automobile engine has a cylinder with a volume of 500.0 \(\mathrm{mL}\) that is filled with air \((21 \%\) oxygen) at a tempera- ture of \(55^{\circ} \mathrm{C}\) and a pressure of 101.0 \(\mathrm{kPa}\) . What mass of octane must be injected to react with all of the oxygen in the cylinder? $$2 \mathrm{C}_{8} \mathrm{H}_{18}(l)+25 \mathrm{O}_{2}(g) \rightarrow 16 \mathrm{CO}_{2}(g)+18 \mathrm{H}_{2} \mathrm{O}(g)$$

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