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A gas is stored in a sealed container of constant volume. The temperature of the gas increases.
This causes the pressure of the gas to increase
What happens to the gas molecules during this pressure increase?
A The average kinetic energy of the molecules increases.
B The average separation of the molecules decreases
The average separation of the molecules increases,
с
D
The volume of each molecule increases.

Sagot :

AditiNigam

Answer:

If the gas volume is decreased, the container wall area decreases and the molecule-wall collision frequency increases, both of which increase the pressure exerted by the gas. Avogadro's law. At constant pressure and temperature, the frequency and force of molecule-wall collisions are constant.

Explanation:

As the temperature increases, the average kinetic energy increases as does the velocity of the gas particles hitting the walls of the container. The force exerted by the particles per unit of area on the container is the pressure, so as the temperature increases the pressure must also increase.

As the temperature of the gas increases, the particles gain kinetic energy and their speed increases. This means that the particles hit off the sides more often and with greater force. Both of these factors cause the pressure of the gas to increase.

What is temperature ?

Temperature is a measure of the degree of hotness of a body. The SI unit of temperature is kelvin (K).The instrument used to measure temperature is called a thermometer.

What is kinetic energy ?

Kinetic energy is a form of energy that an object or a particle has by reason of its motion. If work, which transfers energy, is done on an object by applying a net force, the object speeds up and thereby gains kinetic energy.

Know more about kinetic energy here

https://brainly.com/question/5223218

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