Question

According to kinetic theory of gases kinetic energy depends on (1) Temperature (2) Pressure (3) Collision (4) Atomic number

Short answer

The kinetic energy of gas particles depends on temperature.

Step-by-step solution

- Identify the Principle

The kinetic theory of gases states that the kinetic energy of gas particles is directly proportional to the temperature of the gas.

- Review the Options

Look at the given options: (1) Temperature, (2) Pressure, (3) Collision, and (4) Atomic number, and see which one aligns with the kinetic theory of gases.

- Eliminate Irrelevant Options

Pressure, collision, and atomic number do not directly affect the kinetic energy of gas particles based on kinetic theory. Eliminate options (2), (3), and (4).

- Conclude the Correct Answer

Since according to the kinetic theory of gases, the kinetic energy is dependent on temperature, the correct answer is (1) Temperature.

Key concepts

kinetic theory of gases

The kinetic theory of gases explains the behavior of gases by treating them as a large number of small particles in constant, random motion. This theory makes several key assumptions about gas particles:

• They are in constant, random motion.
• They collide elastically with each other and the walls of the container.
• They do not exert forces on each other except during collisions.

From these assumptions, we can derive several important properties of gases, including pressure, temperature, and volume. The kinetic theory helps us understand why gases expand to fill their containers and why they can be easily compressed. It is also essential for explaining the relationship between the average kinetic energy of gas particles and the temperature of the gas.

temperature

Temperature is a measure of the average kinetic energy of the particles in a substance. In the context of gases, this means that if the temperature of a gas increases, the average kinetic energy of its particles also increases. This is because temperature is directly proportional to kinetic energy. To better understand this, consider the equation for the average kinetic energy of a gas particle: \text{K.E.} = \frac{3}{2}kT\, where \( k \) is the Boltzmann constant and \( T \) is the absolute temperature. This equation shows that the kinetic energy of a gas particle increases as the temperature rises. This relationship highlights the importance of temperature in determining the behavior and properties of gases.

kinetic energy and temperature relationship

The relationship between kinetic energy and temperature is foundational in the kinetic theory of gases. As previously mentioned, the kinetic energy of gas particles is directly proportional to the temperature. This means that when the temperature of a gas increases, the particles move faster due to their increased kinetic energy. Conversely, if the temperature decreases, the kinetic energy of the particles decreases, leading to slower movement. This relationship is crucial for understanding many gas behaviors:

• Higher temperatures result in higher pressures if the volume of the gas is constant because particles collide more frequently and with greater force.
• Gases expand when heated because increased kinetic energy causes particles to move apart more.
• At low temperatures, gases can condense into liquids as particles lose energy and move closer together.

In summary, the direct relationship between kinetic energy and temperature underpins many of the observable properties and reactions of gases.