Respuesta :
The average kinetic energy of the gas's molecules directly relates to its temperature. Faster moving particles will more frequently and violently hit the container walls. Because of this, the force acting on the container's walls increases, increasing the pressure.
What happens when the temperature of a gas is increased?
- We know that temperature is proportional to the average kinetic energy of a sample of gas. The proportionality constant is (2/3)R and R is the gas constant with a value of 0.08206 L atm K-1 mol-1 or 8.3145 J K-1 mol-1.
- The average kinetic energy and the velocity of the gas particles striking the container walls rise as the temperature rises. As the temperature rises, the pressure must as well since pressure is the force the particles per unit of area exert on the container.
- The molecules in a gas gain more energy and can move more quickly as it is heated. The pressure will rise, and there will be greater impacts on the container walls. On the other hand, cooling the molecules will cause them to slow down and lower the pressure.
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When the volume of gas increased the KE of gases particles increases and hit the walls of container which increases the pressure on the walls .
What if gas will increase?
The gas expands in a closed container . The molecules strike and hit each other therefore the pressure at the walls increase.
According to ideal gas law , when volume is cnstant the Pressure and temperature both will increase.
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