Chapter 1: Problem 6
State whether the following statements are true or false. Gases show deviations from ideal behaviour at high temperatures and high pressures.
Short Answer
Expert verified
Based on the analysis of the ideal gas law and the conditions under which gases exhibit ideal behavior, is the following statement TRUE or FALSE: "Gases show deviations from ideal behavior at high temperatures and high pressures."
Answer: FALSE
Step by step solution
01
Understand the ideal gas law
The ideal gas law is represented by the equation PV = nRT, where P is the pressure of the gas, V is the volume, n represents the number of moles, R is the ideal gas constant, and T is the temperature. This equation is valid for an ideal gas, which is a hypothetical gas that obeys the ideal gas law perfectly under all conditions.
02
Recognize conditions for ideal gas behavior
Real gases can approximate ideal behavior under certain conditions, specifically low pressures and high temperatures. Low pressures provide enough space between gas particles for the intermolecular forces to become negligible, while high temperatures allow gas particles to move at higher velocities and their kinetic energies to dominate over intermolecular forces.
03
Analyze the statement about deviations from ideal behavior
Now we can examine the given statement: "Gases show deviations from ideal behavior at high temperatures and high pressures." We've established that gases closely follow ideal behavior at high temperatures and low pressures. However, the statement claims that gases deviate from ideal behavior at high temperatures and high pressures.
04
Determine the validity of the statement
Since we know that gases are more likely to follow ideal behavior when they are at high temperatures and low pressures, the statement which claims that gases deviate from ideal behavior at high temperatures and high pressures is FALSE. The correct statement should say "Gases show deviations from ideal behavior at low temperatures and high pressures," which is when real gases exhibit more significant deviations from ideal behavior due to more substantial intermolecular forces and reduced kinetic energies.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Real Gases
Real gases are natural gases that deviate from the ideal gas law's predictions under certain conditions. Unlike ideal gases, which are hypothetical constructs, real gases have actual volume and intermolecular forces. These forces make real gas behavior more complex and less predictable than the ideal gas law suggests.
Some factors influence real gas behavior:
Some factors influence real gas behavior:
- Intermolecular Forces: These are attractions or repulsions between gas molecules. In ideal gases, these forces are assumed to be nonexistent. However, in real gases, they can significantly affect properties like pressure and volume.
- Volume of Gas Particles: In the ideal gas model, gas particles are considered point particles with no volume. In reality, gas molecules have finite sizes, affecting how they occupy space within a container.
Deviations from Ideal Behavior
Deviations from ideal behavior occur when the assumptions of the ideal gas law do not hold true. Real gases deviate from the ideal gas law under certain conditions—primarily at low temperatures and high pressures.
At low temperatures, the kinetic energy of gas particles decreases, making intermolecular forces more significant. As a result, these attractive forces can cause gases to condense into liquids or solids, creating deviations from ideal predictions.
At high pressures, gas particles are forced closer together, increasing the effect of intermolecular forces and the volume occupied by the gas molecules themselves. This can lead to deviations from the ideal law, where the predicted volume is not accurate.
This behavior leads to the Boyle Temperature, a specific temperature at which a real gas behaves ideally over a range of pressures, providing further insight into how temperature affects real gas behavior.
At low temperatures, the kinetic energy of gas particles decreases, making intermolecular forces more significant. As a result, these attractive forces can cause gases to condense into liquids or solids, creating deviations from ideal predictions.
At high pressures, gas particles are forced closer together, increasing the effect of intermolecular forces and the volume occupied by the gas molecules themselves. This can lead to deviations from the ideal law, where the predicted volume is not accurate.
This behavior leads to the Boyle Temperature, a specific temperature at which a real gas behaves ideally over a range of pressures, providing further insight into how temperature affects real gas behavior.
High Pressure and Temperature Effects
The behavior of gases under high pressure and temperature is quite distinct. Under these conditions, gases can show significant deviations from what the ideal gas law predicts. However, it's crucial to differentiate how these factors, pressure, and temperature, individually influence gas behavior.
- High Pressure: Increases in pressure can lead to greater proximity between gas molecules, thereby enhancing intermolecular attractions. This proximity can make the gas behave less ideally as pressure increases, as the available space becomes less than the calculated ideal values.
- High Temperature: At elevated temperatures, gases generally behave more ideally. The increased kinetic energy causes gas molecules to overcome intermolecular attractions, making these forces negligible. However, if both high pressure and high temperature are present, the effects can be complex and less predictable, often requiring more sophisticated models than the ideal gas law.