Question

The closest distancc betwecn the centres of two molcculcs of a gas taking part in collision is called (1) collision diameter (2) collision number (3) molecular diameter (4) both 1 and 3

Short answer

Both (1) collision diameter and (3) molecular diameter.

Step-by-step solution

Understand the definition

Read the given statement carefully. The closest distance between the centers of two molecules of a gas taking part in a collision is described.

Identify key terms

Identify the key term from the options provided that matches the definition. The term that describes the closest distance between centers of colliding molecules is sought.

Match the definition to options

Review each option: (1) collision diameter, (2) collision number, (3) molecular diameter, and (4) both 1 and 3. Determine which term fits the definition provided.

Evaluate each option

Evaluate: Collision diameter refers to the shortest distance between the centers of colliding molecules. Collision number is the number of collisions. Molecular diameter is a similar concept, but it can also just mean the diameter of a single molecule.

Confirm the answer

Since collision diameter specifically addresses the shortest distance between centers of colliding molecules, it fits the definition accurately. Also, molecular diameter could be relevant but not as precisely as collision diameter within the context of two colliding molecules.

Key concepts

Gas Molecule Collision

Gas molecule collisions are fundamental to understanding the behavior of gases. When gas molecules collide, they transfer energy and momentum, impacting properties like pressure and temperature.
In a gas, molecules move in random directions and with various speeds. When they collide, these interactions are typically elastic, meaning there is no loss of kinetic energy.
This is central to the Kinetic Theory of Gases.
The frequency and nature of these collisions are described using terms such as 'collision diameter' and 'collision number.'
Key points to remember:

• Gas molecule collisions are essential for explaining gas properties.
• They are typically elastic, conserving kinetic energy.
• 'Collision diameter' is the closest distance between two colliding molecules' centers.
• 'Collision number' refers to the number of collisions happening in a given time.

These concepts help us understand how gases behave under different conditions.

Molecular Interaction

Molecular interactions refer to the ways in which molecules influence each other's behavior. In gases, these interactions are primarily through collisions.
During a collision, molecules come very close to each other, up to their 'collision diameter', which is a measure of the effective distance at which they interact.
This distance is crucial in determining how often collisions occur. Key aspects include:

• Molecular interactions determine how energy and momentum are transferred.
• 'Collision diameter' plays a vital role in these interactions.
• Understanding these interactions helps in predicting gas behavior under various environments.

By understanding molecular interactions, we gain insights into the microscopic events that shape macroscopic properties like pressure and temperature.

Kinetic Theory of Gases

The Kinetic Theory of Gases provides a framework to understand the behavior of gases. It postulates that gas molecules are in constant, random motion, colliding elastically.
Several key assumptions form this theory:

• Molecules are small compared to the distances between them.
• There are no intermolecular forces except during collisions.
• Collisions are perfectly elastic, meaning no kinetic energy is lost.

One important concept in this theory is the 'collision diameter'. This measures the closest distance between the centers of two colliding molecules. Another is the idea of molecular velocity distribution, which follows Maxwell-Boltzmann statistics.
The theory helps explain observable gas properties like temperature, which relates to the average kinetic energy of the molecules, and pressure, resulting from collisions with container walls.
The Kinetic Theory of Gases unifies these concepts to describe and predict gas behavior across a range of conditions.