Compare the kinetic energy of molecules at high and low temperatures.
High Temperature: Molecules have higher average kinetic energy and move faster. | Low Temperature: Molecules have lower average kinetic energy and move slower.
Differentiate between successful and unsuccessful collisions in a chemical reaction.
Successful Collisions: Have proper orientation and sufficient energy to overcome the activation energy. | Unsuccessful Collisions: Lack proper orientation or sufficient energy.
What is the effect of increasing temperature on the rate of a reaction, according to collision theory?
Increasing temperature increases the average kinetic energy of molecules, leading to more frequent and forceful collisions, thus increasing the reaction rate.
What is the effect of a catalyst on the activation energy of a reaction?
A catalyst lowers the activation energy of a reaction.
What is the effect of improper orientation during a molecular collision?
If molecules collide with improper orientation, they will not react, even if they possess sufficient energy.
What happens when two objects reach thermal equilibrium?
There is no net heat transfer between the objects, and they have the same temperature.
Define temperature in terms of molecular motion.
Temperature is a measure of the average kinetic energy of particles.
What is activation energy?
The minimum kinetic energy required for a collision to result in a chemical reaction.
Define thermal equilibrium.
The state where two objects have the same temperature, and there is no net heat transfer between them.
What is the collision theory?
A theory stating that for a chemical reaction to occur, reactant molecules must collide with sufficient energy and proper orientation.
State the Zeroth Law of Thermodynamics.
If object A is in thermal equilibrium with object B, and object B is in thermal equilibrium with object C, then object A is also in thermal equilibrium with object C.
