Real vs Ideal Gases Quiz

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Questions and Answers

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?

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?

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?

The volume occupied by the gas particles. Signup and view all the answers

Which condition is likely to cause real gases to behave less ideally?

Low temperatures and high pressures. Signup and view all the answers

What happens to the average kinetic energy of gas molecules if volume is reduced without changing temperature?

It remains unchanged. Signup and view all the answers

According to Boyle's Law, what relationship exists between pressure and volume at constant temperature?

Pressure is inversely proportional to volume. Signup and view all the answers

How does an increase in gas temperature affect the pressure of the gas at constant volume according to Gay-Lussac's Law?

Pressure increases. Signup and view all the answers

What occurs to the volume of gas when temperature increases if pressure is to remain constant?

Volume increases. Signup and view all the answers

What specific conditions must be met to compare the rates of effusion of two gases according to Graham’s Law?

Same pressure and same temperature. Signup and view all the answers

Which of the following describes ideal gases as opposed to real gases?

They do not interact with each other. Signup and view all the answers

Which of the following describes the effect on kinetic energy when two gases with the same temperature are compared?

They have identical average kinetic energies. Signup and view all the answers

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?

Doubles. Signup and view all the answers

What is the relationship between the average kinetic energy and temperature according to the kinetic molecular theory?

Temperature is directly proportional to average kinetic energy. Signup and view all the answers

According to the kinetic molecular theory, how do gas molecules behave?

Gas molecules are in constant random motion in straight lines. Signup and view all the answers

What does the effusion rate ratio of ammonia to hydrogen chloride indicate?

Ammonia effuses 1.463 times faster than hydrogen chloride. Signup and view all the answers

Which statement about the collision between gas molecules is correct?

Collisions are perfectly elastic. Signup and view all the answers

What is the relationship between pressure and gas particle collisions with the container walls?

Pressure is due to the net effect of collisions with the walls. Signup and view all the answers

In the context of kinetic molecular theory, what does the negligible volume of gas particles imply?

The volume of gas particles is negligible compared to the volume of the gas container. Signup and view all the answers

What does the equation $PV \alpha average KE$ signify in the kinetic molecular theory?

The product of pressure and volume is related to average kinetic energy. Signup and view all the answers

Which of the following assumptions is NOT part of the kinetic molecular theory?

Gas particles experience significant interaction with each other. Signup and view all the answers

What is the main difference between diffusion and effusion?

Diffusion involves complete intermingling of gases, whereas effusion involves movement through a tiny hole into lower pressure. Signup and view all the answers

According to Graham's law, how does the rate of effusion relate to the density of a gas?

The rate of effusion increases as the density of a gas decreases. Signup and view all the answers

Under which condition is the kinetic energy of two different gases the same?

At constant pressure and temperature. Signup and view all the answers

Which formula correctly represents the relationship between effusion rate and formula mass?

Effusion rate is inversely proportional to the square root of the formula mass. Signup and view all the answers

What is the expression for kinetic energy of a gas molecule?

K.E = ½ mv^2 Signup and view all the answers

What happens to the effusion rate of a gas when its molecular weight increases?

Effusion rate decreases. Signup and view all the answers

How is the density of a gas related to its formula mass?

Density is directly proportional to formula mass. Signup and view all the answers

If two gases, A and B, have different effusion rates, how does their formula mass relate to their rates?

The effusion rate of a gas is inversely proportional to the square root of its formula mass. Signup and view all the answers

Study Notes

Lecture No. 3: Properties of Gases (2)

Diffusion: The complete spreading out and mixing of one gas among another. Examples include perfume spreading through the air.
Effusion: The movement of gas molecules through a very small opening into a region of lower pressure.

Graham's Law of Effusion

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.
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.
effusion rate(A) / effusion rate(B) = √(d_B/d_A )
Constant: Effusion rate × √density = constant (approximately the same for all gases.)

Kinetic Energy

Definition: The energy of motion. All moving objects and particles have kinetic energy.
Formula: K.E. = ½ m∙v²
m = mass
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.