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What are the 5 postulates of the KMT?
The Kinetic Molecular Theory (KMT) is based on five postulates: Matter is composed of a large number of small particles (atoms or molecules) that are in constant motion. These particles move in straight lines until they collide with each other or with the walls of their container. The collisions between particles are perfectly elastic, meaning there is no loss of kinetic energy. The average kinetic energy of the particles is directly proportional to the temperature of the gas in Kelvin. There are no attractive or repulsive forces between the particles, and the volume of the particles themselves is negligible compared to the volume of the gas.
What are five ways to affect rxn rates?
Reaction rates can be affected by several factors: Concentration: Increasing the concentration of reactants typically raises the reaction rate due to more frequent collisions between molecules. Temperature: Raising the temperature generally increases reaction rates as higher thermal energy leads to more energetic collisions. Surface Area: For solid reactants, increasing the surface area (e.g., by grinding) enhances the rate by allowing more collisions. Catalysts: Introducing a catalyst lowers the activation energy, speeding up the reaction without being consumed. Pressure: In reactions involving gases, increasing pressure can increase the reaction rate by forcing gas molecules closer together, leading to more collisions.
What is the difference between a straight line and a line?
A straight line is the shortest distance between two points, a line is the delineation of a connection between two or more points.
What is the definition of a straight line?
The shortest distance between two points is... a straight line.
What is the difference between a circlee and an ellipse?
A circle is perfectly round and an ellipse is oval.
Assumption of kinetic theory of gas?
The volume occupied by gas molecules is negligible when compared to volume occupied by the gas.The collisions between gas molecules-gas molecules and gas molecules-walls of the container are perfectly elastic.
Are collisions more common between gas molecules or liquid molecules?
Liquids. There are more collisions, but the majority are at lower energies.
All collisions between gas particles are considered to be perfectly what?
All collisions between gas particles are considered to be perfectly elastic, meaning there is no loss of kinetic energy during the collision. This assumption allows for the conservation of momentum and energy to be applied to gas particle interactions.
Are collisions between solvent molecules and solute are more frequent at lower or higher temperatures?
Collisions between solvent molecules and solute are more frequent at higher than lower temperatures.
What a temperature increases affect collisions between molecules?
thermal effect
How does this increase the rate of the reaction?
It increases the number of collisions between molecules. :)
What does collisions mean in gas?
In the context of gases, collisions refer to the interactions between gas molecules or between gas molecules and the walls of the container. These collisions result in changes in the motion and energy of the gas particles, leading to phenomena like pressure and temperature changes. The frequency and intensity of collisions impact the properties and behavior of the gas.
What happenes to the particels of a gas when there are fewer of them?
This is the ideal gas with no collisions between molecules..
How do you increase the number of collisions between molecules?
heating, stirring, surface area
Which describes the path of a gas particle between collisions with other particles?
Straight line
What makes more molecules collide with each other?
Increasing the concentration of the molecules or raising the temperature can both increase the frequency of molecular collisions. Additionally, decreasing the volume of the container can also lead to more collisions between molecules.
Gas pressure is caused by collisions between?
Gas molecules and the walls of the container they are in.
