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Chapter 5: Problem 77

Give two pieces of evidence to show that gases do not behave ideally under all conditions.

Short Answer

Expert verified
Gases deviate from ideal behavior at high pressures and low temperatures.

Step by step solution

01

Understanding Ideal Gas Assumptions

Ideal gas behavior is based on the assumptions that gas particles have negligible volume and do not exert any forces on each other. These are realistic assumptions under high temperature and low pressure conditions.
02

Analyzing Non-Ideal Behavior at High Pressure

Under high pressure conditions, gas particles are forced close together. This proximity increases the interactions between particles and the volume of the gas particles becomes significant. Thus, the assumption of negligible volume and no intermolecular forces is violated.
03

Analyzing Non-Ideal Behavior at Low Temperature

At low temperatures, the kinetic energy of gas particles decreases, allowing attractive forces to become more prominent. These interactions lead to deviations from ideal behavior because the force exerted by nearby particles can no longer be ignored.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Non-ideal Gas Behavior
Gases do not always behave in the ideal manner that textbooks often describe. The concept of ideal gas behavior relies on certain assumptions. It presumes that gas particles move randomly without interacting with each other through any forces. It also assumes that these particles occupy no significant volume. When real-world conditions differ from these assumptions, the behavior of gases deviates from the ideal model.
For instance:
  • At higher pressures, the distance between gas molecules decreases, leading to significant inter-particle forces.
  • At low temperatures, reduced kinetic energy allows these forces to have a noticeable impact.
These deviations are crucial in understanding the realistic behavior of gases in various conditions.
Gas Behavior at High Pressure
When gases are subjected to high pressure, their behavior markedly shifts from ideal. Imagine compressing a gas into a small container鈥攁 situation where the particles are forced to occupy a smaller volume. This proximity increases the likelihood that gas particles will collide with each other more frequently. As a result:
  • The volume of the particles themselves becomes significant.
  • Intermolecular forces, which are ignored in ideal gas assumptions, become more apparent and impactful.
In simple terms, high pressure forces gas particles to behave in ways not accounted for in the ideal gas law. Hence, making corrections for these non-ideal conditions is essential for accurate predictions and calculations.
Gas Behavior at Low Temperature
At low temperatures, gases behave differently compared to ideal predictions due to reduced kinetic energy among the particles. When the energy is lower, particles move more slowly and are more likely to linger near each other. As a result:
  • Attractive forces between particles become more significant, even if weak.
  • The slowing down of velocities increases the impact of these forces.
In cold conditions, the significant effect of these forces leads to deviations from ideal gas behavior. The gas particles no longer act independently, contrary to the assumptions of the ideal gas law. Understanding these differences is vital for applications ranging from industrial processes to the study of atmospheric phenomena.

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Most popular questions from this chapter

In the metallurgical process of refining nickel, the metal is first combined with carbon monoxide to form tetracarbonylnickel, which is a gas at \(43^{\circ} \mathrm{C}\) : $$\mathrm{Ni}(s)+4 \mathrm{CO}(g) \longrightarrow \mathrm{Ni}(\mathrm{CO})_{4}(g)$$ This reaction separates nickel from other solid impurities. (a) Starting with \(86.4 \mathrm{~g}\) of \(\mathrm{Ni}\), calculate the pressure of \(\mathrm{Ni}(\mathrm{CO})_{4}\) in a container of volume \(4.00 \mathrm{~L}\). (Assume the above reaction goes to completion.) (b) On further heating the sample above \(43^{\circ} \mathrm{C},\) it is observed that the pressure of the gas increases much more rapidly than predicted based on the ideal gas equation. Explain.

Why is mercury a more suitable substance to use in a barometer than water?

A gas-filled balloon having a volume of \(2.50 \mathrm{~L}\) at \(1.2 \mathrm{~atm}\) and \(25^{\circ} \mathrm{C}\) is allowed to rise to the stratosphere (about \(30 \mathrm{~km}\) above the surface of Earth), where the temperature and pressure are \(-23^{\circ} \mathrm{C}\) and \(3.00 \times 10^{-3}\) atm, respectively. Calculate the final volume of the balloon.

Assuming that air contains 78 percent \(\mathrm{N}_{2}, 21\) percent \(\mathrm{O}_{2},\) and 1 percent \(\mathrm{Ar},\) all by volume, how many molecules of each type of gas are present in \(1.0 \mathrm{~L}\) of air at STP?

A 6.11 -g sample of a Cu-Zn alloy reacts with \(\mathrm{HCl}\) acid to produce hydrogen gas. If the hydrogen gas has a volume of \(1.26 \mathrm{~L}\) at \(22^{\circ} \mathrm{C}\) and \(728 \mathrm{mmHg}\), what is the percent of \(\mathrm{Zn}\) in the alloy? (Hint: Cu does not react with \(\mathrm{HCl} .\)
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