1. Law of Conservation of Energy The law of conservation of energy states that energy cannot be created or destroyed, only transferred or transformed from one form to another. The total energy in an isolated system remains constant over time. 2. Interaction of Hot Brick and Cold Water a. What happens if a hot brick is placed in a cold bucket of water? The hot brick will transfer heat to the cold water until thermal equilibrium is reached. b. Assuming no energy is lost to the surroundings, how does the temperature of the brick compare with the temperature of the water after some time has passed? The temperature of the brick and the water will be the same after some time has passed, assuming no heat is lost to the surroundings. c. Which substance absorbed energy? The cold water absorbed energy. d. Which substance released energy? The hot brick released energy. 3. Endothermic and Exothermic Processes Endothermic Process: An endothermic process absorbs energy from its surroundings in the form of heat. Exothermic Process: An exothermic process releases energy to its surroundings in the form of heat. 4. Classifying Processes a. Ice melting Endothermic b. Water vapor condensing Exothermic c. Gasoline burning Exothermic d. Rubbing alcohol evaporating Endothermic e. A metal spoon getting hot as it sits in a cup freshly poured tea Exothermic (from the tea's perspective, heat is transferred to the spoon) 5. Specific Heat Capacity vs. Heat Capacity Specific Heat Capacity: The amount of heat energy required to raise the temperature of one gram of a substance by one degree Celsius. Heat Capacity: The amount of heat energy required to raise the temperature of a given quantity (mass) of a substance by one degree Celsius. Difference: Specific heat capacity is an intensive property that does not depend on the amount of substance, whereas heat capacity is an extensive property that depends on the amount of substance. 6. Comparing Specific Heat Capacities Since Substance A increases in temperature more than Substance B for the same amount of absorbed heat energy, Substance A has a lower specific heat capacity compared to Substance B. 7. Energy in Chemical Bonds When chemical bonds are broken, energy is absorbed. When chemical bonds are formed, energy is released. 8. Exothermic Reaction Energy In an exothermic reaction, the energy stored in the reactants is greater than the energy stored in the products. 9. Reaction Energy Change a. Is the reaction exo- or endothermic? Explain. The reaction is endothermic because the temperature of the mixture drops, indicating that energy is absorbed from the surroundings.

Triple Point

Triple Point

The unique combination of pressure and temperature at which a pure substance can coexist in all three phases (solid, liquid, gas) simultaneously.

PT Diagram

A graphical representation showing the relationship between the phases of a substance in terms of pressure and temperature.

Vacuum Chamber

A sealed container used to create low-pressure environments for scientific experiments.

Experiment Setup

The arrangement of equipment and procedures used to investigate phenomena under controlled conditions.

Deposition

The process in which a substance transitions directly from the vapor phase to the solid phase without passing through the liquid phase.

Sulfuric Acid

A compound used to attract water molecules from the gas phase, aiding in improving the vacuum in experiments.

Frost

The formation of ice crystals on surfaces due to the direct deposition of water molecules from the vapor phase.