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When will a collision lead to a chemical reaction?
When the collision is hard and fast enough. Increasing the kinetic energy will increase the likelihood of hard and fast collisions, which will ultimately increase the rate of the reaction. (This is called collision theory.)
How is the activation energy related to whether or not collision between molecules is successful?
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
According to the collision theory what are the two ways to make a reaction go faster?
To make a reaction go faster according to the collision theory, you can either increase the frequency of collisions between reactant particles by raising the temperature or increasing the concentration of reactants, or increase the energy of collisions by raising the temperature of the reaction.
At a constant pressure how does a volume of gas vary with respect to the absolute temperature?
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.
Temperature is relative to the energy of the molecules?
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.
Why does increasing the temperature of a reaction increase its rate?
It provides energy to overcome the activation energy.
When will a collision lead to a chemical reaction?
When the collision is hard and fast enough. Increasing the kinetic energy will increase the likelihood of hard and fast collisions, which will ultimately increase the rate of the reaction. (This is called collision theory.)
How do the factors of temperature and surface area affect the rate of chemical reactions?
Temperature affects the rate of chemical reactions by increasing the speed at which molecules move and collide, leading to more successful collisions. A larger surface area allows for more contact between reactant molecules, increasing the chance of collision and reaction. Both factors can increase reaction rates by promoting collisions between reactant molecules.
Why is Heat transfered between two substances that are in contact is called conduction?
Heat transfer between two substances in contact is called conduction because it occurs through direct contact between molecules. In conduction, heat energy is transferred from higher temperature molecules to lower temperature molecules due to their collision and interaction, leading to an equalization of temperature between the substances.
What does the motion and collision between molecules cause?
Energy.
How is the activation energy related to whether or not collision between molecules is successful?
Generally speaking, the lower the activation energy, the more successful collision between molecules will happen.
According to the collision theory what are the two ways to make a reaction go faster?
To make a reaction go faster according to the collision theory, you can either increase the frequency of collisions between reactant particles by raising the temperature or increasing the concentration of reactants, or increase the energy of collisions by raising the temperature of the reaction.
What effect does an increase in temperature have on the movement of molecules?
An increase in temperature causes molecules to move faster and with greater energy. This results in an increase in the rate of collisions between molecules, leading to higher kinetic energy and an overall increase in the speed of molecular movement.
At a constant pressure how does a volume of gas vary with respect to the absolute temperature?
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.
Temperature is relative to the energy of the molecules?
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.
Why does a substance's temperature increase when it receives more thermal energy?
When a substance receives more thermal energy, its molecules gain kinetic energy and move faster, which causes an increase in temperature. The increased movement and collisions between molecules lead to a rise in temperature.
If you increase the temperature of a gas what happens to the movement of the molecules?
Increasing the temperature of a gas causes the molecules to move faster on average, which leads to an increase in their kinetic energy. This results in more frequent and higher energy collisions between the molecules.
