The number of collisions with enough energy to react increases.
Changes in temperature and activation energy have opposite effects on reaction rate (apex)
The relationship between temperature and molecule movement is a direct variation. Whenever the molecule movement increases so does the temperature; when the molecule movement decreases so does the temperature. I hope that helps.
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
Increasing temperature will increase molecular speed.An object with less massive molecules will have higher molecular speed at the same temperature.When kinetic temperature applies, two objects with the same average translational kinetic energy will have the same temperature. An important idea related to temperature is the fact that a collision between a molecule with high kinetic energy and one with low kinetic energy will transfer energy to the molecule of lower kinetic energy.
It doesn't. The equation for mean free path is: mfp = 1 / [sqrt(2)*n*pi*d^2] In the above equation, n is the number of molecules per unit volume, and d is what is known as the collision diameter (the distance between the centers of the two colliding molecules). Thus, there are only three variables which affect mean free path: number of molecules, volume, and collision diameter. Volume can be changed by a change in temperature, but this question assumes constant volume (meaning pressure will change as temperature changes). As long as the amount of gas is unchanged, the mean free path will be unaffected by changes in temperature. This is a wrong answer. The collision diameter decreases with the increase of temperature.
increased temperture causes rate or reaction to increase.
It provides energy to overcome the activation energy.
Energy.
The relationship between temperature and molecule movement is a direct variation. Whenever the molecule movement increases so does the temperature; when the molecule movement decreases so does the temperature. I hope that helps.
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
Increasing the temperature will cause there to be an increase in kinetic energy. This results in an increase in collision frequency, and eventually an increase in rate of reaction as well.
Increasing temperature will increase molecular speed.An object with less massive molecules will have higher molecular speed at the same temperature.When kinetic temperature applies, two objects with the same average translational kinetic energy will have the same temperature. An important idea related to temperature is the fact that a collision between a molecule with high kinetic energy and one with low kinetic energy will transfer energy to the molecule of lower kinetic energy.
It doesn't. The equation for mean free path is: mfp = 1 / [sqrt(2)*n*pi*d^2] In the above equation, n is the number of molecules per unit volume, and d is what is known as the collision diameter (the distance between the centers of the two colliding molecules). Thus, there are only three variables which affect mean free path: number of molecules, volume, and collision diameter. Volume can be changed by a change in temperature, but this question assumes constant volume (meaning pressure will change as temperature changes). As long as the amount of gas is unchanged, the mean free path will be unaffected by changes in temperature. This is a wrong answer. The collision diameter decreases with the increase of temperature.
Links between chemical entities (atoms or molecules) are quickly destroyed if the temperature increase.
The atoms have greater kinetic energy and move faster when the temperature is raised, resulting in more frequent contact between the magnesium atoms and acid molecules, which will cause the rate of the reaction to increase.
as the temperature increase the molecular interaction between the liquids molecules are weaker, since hydrogen bond is the main factor for association between two molecules which are very weak bond, so it can be break easily when the temperature increase leading to decrease in surface tension
In general, as temperature rises, so does reaction rate. This is because the rate of reaction is dependent on the collision of the reacting molecules or atoms. As temperature rises, molecules or atoms respond with increased motion, increasing the collision rate, thus increasing the reaction rate.
When heat is supplied the intermolecular/interparticulate force decreases and the particles gain in Kinetic energy and start moving randomly. Since, the force between molecules decreases, the intermolecular spaces increase and particles start pressing against the wall of the container in order to escape out.