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What does the constant collision of gas molecules against the inside walls of a container produce A Temperature Bdensity C Pressure Ddiffusion?
Wiki User
∙ 9y ago
The constant collision of gas molecules against the inside walls of a container produces pressure which is directly proportional to the number of collisions.
Wiki User
∙ 9y ago
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The collision of the molecules of a fluid inside the surface of their container best describes?
The collision of the molecules of a fluid inside the surface of their container best describes pressure.
Is the temperature of a gas a measure of how hard its molecules hit the walls of its container?
no
Why would a sealed container of air be crushed after being frozen?
A sealed container of air would be crushed after being frozen because as the pressure decreases, the temperature also decreases. The air molecules inside of the sealed container shrink when it is frozen. The colder the air, the lower the temperature.
Does the collision of molecules create heat?
The number of collisions with enough energy to react increases.
What makes an increase in temperature change the reactions rate?
It increases the collisions that result in a reaction. or it increases the kinetic energy of the molecules.
The collision of the molecules of a fluid inside the surface of their container best describes?
The collision of the molecules of a fluid inside the surface of their container best describes pressure.
What is pressure of gas due to?
collision of air molecules with the walls of the container
What does the constant collision of gas molecules against the inside walls of a container produce?
Pressure and heat.
Why increasing the temperature of a gas in a closed rigid container causes the pressure in the container to increase?
At the molecular scale, increasing the temperature means that the gas molecules are more energetic and are impacting the walls of the container with more momentum, thus imparting more force to the wall per collision. At the macroscopic scale, the ideal gas law is PV = nRT, which tells us that pressure rises linearly with temperature at constant volume.
Why increasing the temperature of a gas in a closed rigid container causes pressure in the container to increase?
At the molecular scale, increasing the temperature means that the gas molecules are more energetic and are impacting the walls of the container with more momentum, thus imparting more force to the wall per collision. At the macroscopic scale, the ideal gas law is PV = nRT, which tells us that pressure rises linearly with temperature at constant volume.
Is the temperature of a gas a measure of how hard its molecules hit the walls of its container?
no
High pressure gases?
when the collision between the gas molecules and the container in which the gas exist is very high.....then the pressure of the gas is very high
How the temperature of gas is increased and decreased?
When the speed of a gas molecules increases, the gas molecules hit their container more often. The more frequently the gas impacts the container walls, the higher the pressure. So, as temperature increases, the pressure also increases.
What happens to molecules as their kinetic energy increases?
They move faster, number of collision increases,also the temperature increases.
What will happen to the kinetic energy of gas molecules trapped in a rigid container if the temperature is increased?
increased
Is there any collision of molecules in diffusion?
There is constantly collision of molecules no matter what process they are going through
How does the temperature of an object change when its molecules colide?
The temperature of the gas is proportional to the average kinetic energy of its molecules. Faster moving particles will collide with the container walls more frequently and with greater force. This causes the force on the walls of the container to increase and so the pressure increases.
