0
What happens to the pressure in number of collisions as the volume is decreased in the image above?
Wiki User
∙ 8y agoWant this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
What is the outcome of decreasing the numbers of collisions of gas particles per unit area within a container?
Decreasing the number of collisions of gas particles per unit area within a container would result in a decrease in pressure inside the container. This is because pressure is directly proportional to the number of collisions of gas particles on the walls of the container. As the collisions decrease, the pressure exerted by the gas decreases as well.
What happens to pressure on the molecule level when the number of moles of gas is increased at constant volumeWhat happens to the number of collisions with the side of the container?
When the number of moles of gas is increased at constant volume, the pressure on the molecule level increases because there are more gas particles colliding with the walls of the container. This is because there are more gas molecules in the same volume, leading to more frequent collisions with the sides of the container.
Does increasing pressure affect reaction rate?
If the pressure increase the number of intermolecular collisions increase and so the reaction rate. This is valid for gases.
What happens to the temperature increase the number of particles what happens to the pressure?
Increasing the temperature the number of particles remain constant and the pressure increase.
Why does increasing the pressure of a gas increase the reaction time?
The explanation is: increasing the pressure is equal to an increasing of concentration of reactants.In a concentrated environment the possibility of interactions between molecules is higher.And the consequence of more collisions is the increasing of reaction rate.
What happens to the average kinetic energy of the particles the pressure and number of collisions when the temperature is decreased?
When the temperature is decreased, the average kinetic energy of particles decreases since temperature is directly related to the average kinetic energy of particles. As a result, the pressure and number of collisions between particles will also decrease because particles will have less energy to move and collide with each other.
What happens when the pressure of a gas is decreased?
When the pressure of a gas is decreased, the gas molecules move farther apart, leading to an increase in volume. This can cause the gas to expand and fill a larger space. Additionally, decreasing pressure can also lower the temperature of the gas due to the reduced number of molecular collisions.
What happens to the pressure of a system when the volume is decreased if the temperature and number of gas particles are held constant according to Boyles Law?
According to Boyle's Law, if the volume of a gas is decreased while keeping the temperature and number of gas particles constant, the pressure of the gas will increase. This is because there is less space for the gas particles to occupy, leading to more frequent collisions with the walls of the container, resulting in an increased pressure.
Why does increasing the pressure of a gas increase the pressure rate?
It increases the number of collisions.
How does pressure volume density and temperature affect diffusion?
An increase in pressure and temperature generally increases the rate of diffusion by increasing the kinetic energy of the particles, leading to more frequent collisions and a higher probability of diffusion. However, an increase in volume density can hinder diffusion by increasing the number of particles in a given space, which can lead to more collisions and decreased diffusion rates.
What happens to pressure on the molecule level when the number of moles of gas is increased at constant volumeWhat happens to the number of collisions with the side of the container?
When the number of moles of gas is increased at constant volume, the pressure on the molecule level increases because there are more gas particles colliding with the walls of the container. This is because there are more gas molecules in the same volume, leading to more frequent collisions with the sides of the container.
Why does an increase in the number of molecules increase the pressure?
An increase in the number of molecules increases the frequency of molecular collisions with the container walls. With more collisions per unit time, the average force exerted by the molecules on the walls increases, resulting in an increase in pressure.
Why does lowering the pressure make there less collisions?
Lowering the pressure decreases the number of gas molecules in a given volume, leading to fewer collisions because there are fewer particles available to collide with each other. As a result, the chances of collisions occurring are reduced when the pressure is lowered.
What happens to a fraction if its denominator is increased or decreased?
If a fraction's denominator is increased, the number gets smaller. If a fraction's denominator is decreased, the number gets bigger.
How does pressure affect reaction rates?
If the pressure increase the number of intermolecular collisions increase and so the reaction rate. This is valid for gases.
Why does a gas exert more pressure if it's volume is reduced?
As the volume is decreased, the same number of molecules of air have a smaller space to move freely in. The number of collisions of molecules of air with the walls of the container per unit time increases. Since pressure is the force exerted over an area, the pressure increases.
What happens to air pressure if more air molecules are added to a balloon?
Adding more air molecules to a balloon increases the number of collisions between the molecules and the balloon walls, thereby increasing the pressure inside the balloon. This increase in air pressure causes the balloon to expand until the pressure inside matches the pressure outside.
