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Questions and Answers
What distinguishes real gases from ideal gases?
What distinguishes real gases from ideal gases?
- Real gases are affected by intermolecular attractive forces. (correct)
- Real gases always behave according to the Ideal Gas Law.
- Real gases occupy no volume.
- Real gases have higher compressibility than ideal gases.
Why is the Ideal Gas Law not applicable to real gases?
Why is the Ideal Gas Law not applicable to real gases?
- Real gases can be approximated as solids at high pressure.
- Real gases have a fixed amount of energy.
- Real gases do not have any mass.
- Real gases have significant intermolecular forces and occupy measurable volume. (correct)
Which of the following is a feature of the Van der Waals equation?
Which of the following is a feature of the Van der Waals equation?
- It accounts for the volume occupied by gas molecules. (correct)
- It cannot be used for ideal gases.
- It simplifies to the Ideal Gas Law at high temperatures. (correct)
- It is only applicable to solids.
In the Van der Waals equation, what does the term 'nb' represent?
In the Van der Waals equation, what does the term 'nb' represent?
Which condition is likely to cause real gases to behave less ideally?
Which condition is likely to cause real gases to behave less ideally?
What happens to the average kinetic energy of gas molecules if volume is reduced without changing temperature?
What happens to the average kinetic energy of gas molecules if volume is reduced without changing temperature?
According to Boyle's Law, what relationship exists between pressure and volume at constant temperature?
According to Boyle's Law, what relationship exists between pressure and volume at constant temperature?
How does an increase in gas temperature affect the pressure of the gas at constant volume according to Gay-Lussac's Law?
How does an increase in gas temperature affect the pressure of the gas at constant volume according to Gay-Lussac's Law?
What occurs to the volume of gas when temperature increases if pressure is to remain constant?
What occurs to the volume of gas when temperature increases if pressure is to remain constant?
What specific conditions must be met to compare the rates of effusion of two gases according to Graham’s Law?
What specific conditions must be met to compare the rates of effusion of two gases according to Graham’s Law?
Which of the following describes ideal gases as opposed to real gases?
Which of the following describes ideal gases as opposed to real gases?
Which of the following describes the effect on kinetic energy when two gases with the same temperature are compared?
Which of the following describes the effect on kinetic energy when two gases with the same temperature are compared?
If the volume of a gas is halved while the temperature remains constant, what will happen to the number of collisions with a unit area?
If the volume of a gas is halved while the temperature remains constant, what will happen to the number of collisions with a unit area?
What is the relationship between the average kinetic energy and temperature according to the kinetic molecular theory?
What is the relationship between the average kinetic energy and temperature according to the kinetic molecular theory?
According to the kinetic molecular theory, how do gas molecules behave?
According to the kinetic molecular theory, how do gas molecules behave?
What does the effusion rate ratio of ammonia to hydrogen chloride indicate?
What does the effusion rate ratio of ammonia to hydrogen chloride indicate?
Which statement about the collision between gas molecules is correct?
Which statement about the collision between gas molecules is correct?
What is the relationship between pressure and gas particle collisions with the container walls?
What is the relationship between pressure and gas particle collisions with the container walls?
In the context of kinetic molecular theory, what does the negligible volume of gas particles imply?
In the context of kinetic molecular theory, what does the negligible volume of gas particles imply?
What does the equation $PV \alpha average KE$ signify in the kinetic molecular theory?
What does the equation $PV \alpha average KE$ signify in the kinetic molecular theory?
Which of the following assumptions is NOT part of the kinetic molecular theory?
Which of the following assumptions is NOT part of the kinetic molecular theory?
What is the main difference between diffusion and effusion?
What is the main difference between diffusion and effusion?
According to Graham's law, how does the rate of effusion relate to the density of a gas?
According to Graham's law, how does the rate of effusion relate to the density of a gas?
Under which condition is the kinetic energy of two different gases the same?
Under which condition is the kinetic energy of two different gases the same?
Which formula correctly represents the relationship between effusion rate and formula mass?
Which formula correctly represents the relationship between effusion rate and formula mass?
What is the expression for kinetic energy of a gas molecule?
What is the expression for kinetic energy of a gas molecule?
What happens to the effusion rate of a gas when its molecular weight increases?
What happens to the effusion rate of a gas when its molecular weight increases?
How is the density of a gas related to its formula mass?
How is the density of a gas related to its formula mass?
If two gases, A and B, have different effusion rates, how does their formula mass relate to their rates?
If two gases, A and B, have different effusion rates, how does their formula mass relate to their rates?
Flashcards
Diffusion
Diffusion
The process where gas molecules spread out and mix evenly with other gas molecules. Think of perfume spreading through the air.
Effusion
Effusion
The process where gas molecules escape through a tiny hole into an area of lower pressure. Imagine air escaping from a punctured balloon.
Graham's Law of Effusion
Graham's Law of Effusion
States that the rates at which gases effuse are inversely proportional to the square root of their densities. Lighter gases effuse faster.
Kinetic Energy
Kinetic Energy
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Effusion Rate / Speed
Effusion Rate / Speed
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Molecular Weight
Molecular Weight
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Density
Density
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Effusion Rate Ratio
Effusion Rate Ratio
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Boyle's Law
Boyle's Law
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Gay-Lussac's Law
Gay-Lussac's Law
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Charles's Law
Charles's Law
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Ideal Gas
Ideal Gas
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Real Gas
Real Gas
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Kinetic Molecular Theory (KMT)
Kinetic Molecular Theory (KMT)
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Random Motion of Gas Particles
Random Motion of Gas Particles
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Kinetic Energy and Temperature
Kinetic Energy and Temperature
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Kinetic Energy (KE)
Kinetic Energy (KE)
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Elastic Collisions of Gas Particles
Elastic Collisions of Gas Particles
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Pressure and Collisions
Pressure and Collisions
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Negligible Volume of gas Particles
Negligible Volume of gas Particles
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Ideal Gas Law and Kinetic Theory
Ideal Gas Law and Kinetic Theory
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Van der Waals Equation
Van der Waals Equation
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Intermolecular Forces
Intermolecular Forces
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Study Notes
Lecture No. 3: Properties of Gases (2)
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Diffusion: The complete spreading out and mixing of one gas among another. Examples include perfume spreading through the air.
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Effusion: The movement of gas molecules through a very small opening into a region of lower pressure.
Graham's Law of Effusion
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Graham's Law: The rate of effusion of gases is inversely proportional to the square root of their densities, at constant pressure and temperature. This means Effusion rate ∝ 1/√d.
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Formula: The effusion rate of gas A divided by the effusion rate of gas B is equal to the square root of the density of gas B divided by the density of gas A.
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effusion rate(A) / effusion rate(B) = √(dB/dA )
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Constant: Effusion rate × √density = constant (approximately the same for all gases.)
Kinetic Energy
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Definition: The energy of motion. All moving objects and particles have kinetic energy.
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Formula: K.E. = ½ m∙v²
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m = mass
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v = velocity or speed
Kinetic Molecular Theory (KMT)
- Explanation: KMT explains macroscopic properties of gases like pressure, temperature, and volume.
- Application: Explains the behavior of ideal gases.
Assumptions of the Kinetic Molecular Gas
- Small Particles: Gases consist of tiny particles (molecules).
- Constant Random Motion: Gas molecules constantly move randomly in straight lines.
- Large Distances: The distance between gas molecules is much larger than the size of the molecules.
- No Interaction: There's negligible interaction between gas molecules (except for occasional collisions).
- Perfectly Elastic Collisions: All collisions between gas molecules are perfectly elastic; no loss of kinetic energy during collisions.
The Average Kinetic Energy and Temperature
- Dependence: The average kinetic energy of the particles depends on the Kelvin temperature
- Pressure: Elastic collisions on the container walls result in pressure.
- Volume: The large spaces between molecules mean the volume of the particles is negligible compared to the container volume.
Kinetic Theory and Gas Laws
- Temperature and Peaks: The peak of a graph (for kinetic energy) shows the highest experienced value, but the average value is slightly higher, due to the lack of symmetry.
- PV Proportional to KE: Based on calculations, the product of pressure and volume (PV) is proportional to the average kinetic energy (KE).
- Ideal Gas Law and Temperature: The ideal gas law (PV = nRT) is related to the average K.E. with respect to temperature(T).
- Pressure-Volume Relationship (Boyle's Law): Reducing the volume of a gas, at constant temperature, increases the pressure. (P1V1 = P2V2)
- Pressure-Temperature Relationship (Gay-Lussac's Law): At fixed volume, an increase in temperature also increases pressure(P1/T1 = P2/T2).
- **Temperature-Volume Relationship (Charles's Law):**At constant pressure, heating up a gas leads to expansion (V1/T1 = V2/T2).
- Effusion Law: Graham's law relates rates of effusion to molecular mass
- Ideal Gases: All gas laws are obeyed by ideal gases under all conditions. Ideal gases consist of small particles, have negligible volume, don't interact, and have perfectly elastic collisions.
- Real Gases: Real gases deviate from ideal behavior due to molecular volume & intermolecular forces; more pronounced at higher pressure & lower temperature. The Van der Waals equation approximates real gas behavior.
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Description
Test your understanding of the differences between real and ideal gases with this quiz. Explore concepts like the Ideal Gas Law and the Van der Waals equation, as well as factors affecting the behavior of gases. Challenge yourself with questions designed to deepen your knowledge of gas laws.
