What is the effect of increasing temperature on the average kinetic energy of particles?
Increasing temperature increases the average kinetic energy of particles.
What happens to the stability of a compound as its potential energy decreases?
The compound becomes more stable.
What happens to the temperature of the surroundings in an exothermic reaction?
The temperature of the surroundings increases.
What happens to the temperature of the surroundings in an endothermic reaction?
The temperature of the surroundings decreases.
What is the effect of increasing the distance between charged particles on electrostatic potential energy?
Increasing the distance decreases the electrostatic potential energy.
Define Kinetic Energy.
Energy of motion.
Define Potential Energy.
Stored energy due to position or composition.
What is Electrostatic Energy?
Potential energy due to the interaction of charged particles.
What is the Law of Conservation of Energy?
Energy cannot be created or destroyed, only transferred or converted.
Define a 'system' in thermodynamics.
The specific part of the universe we're interested in.
Define 'surroundings' in thermodynamics.
Everything else in the universe outside of the system.
What are State Functions?
Properties that depend only on the current state of the system, not how it got there.
Define Enthalpy (H).
The total heat content of a system. It's a state function.
Define Endothermic Process.
Heat is absorbed by the system from the surroundings.
Define Exothermic Process.
Heat is released by the system to the surroundings.
Differentiate between an Open, Closed, and Isolated system.
Open: Exchanges both matter and energy | Closed: Exchanges energy but not matter | Isolated: Exchanges neither matter nor energy.
What are the differences between endothermic and exothermic processes?
Endothermic: Heat absorbed, +ฮH, feels cold | Exothermic: Heat released, -ฮH, feels hot.
Compare and contrast Kinetic and Potential Energy.
Kinetic: Energy of motion, depends on mass and velocity | Potential: Stored energy, depends on position or composition.
Compare State Functions and Non-State Functions.
State Functions: Path independent, depend only on initial and final states (e.g., energy, enthalpy) | Non-State Functions: Path dependent (e.g., heat, work).
