Across
- 2. The change in concentration of reactants or products per unit time, typically expressed in mol/L·s; affected by factors such as temperature, concentration, and catalysts.
- 4. The technique used to measure the amount of heat released or absorbed during a chemical reaction or physical process.
- 5. Collisions between particles that have the proper orientation and sufficient energy to result in a reaction.
- 9. A substance that increases the rate of a chemical reaction by lowering the activation energy required, without being consumed in the reaction itself.
- 10. A chemical reaction that releases heat, causing the temperature of the surroundings to increase; commonly associated with combustion and certain types of oxidation reactions.
- 12. The total heat content of a system, its change is represented by ΔH; it reflects the energy absorbed or released in a chemical reaction under constant pressure.
- 15. A process where a chemical compound breaks down into simpler substances when heated, such as the decomposition of calcium carbonate into calcium oxide and carbon dioxide.
- 17. The amount of energy required to break one mole of bonds in a gaseous molecule, used to calculate enthalpy changes in reactions involving bond breaking and forming.
- 19. A reaction where the rate is proportional to the square of the concentration of one reactant or the product of two reactant concentrations, often written as Rate=k[A]2 or Rate=k[A][B].
- 21. A reaction or process that absorbs heat from its surroundings, resulting in a decrease in temperature of the surroundings, such as the melting of ice.
- 22. A principle stating that the total enthalpy change of a reaction is independent of the pathway it takes, allowing enthalpy changes of multiple reactions to be added algebraically.
Down
- 1. The minimum energy that reactants must possess in order to successfully collide and form products in a chemical reaction; often represented by the symbol Ea.
- 3. A detailed, step-by-step description of the pathway taken by molecules during a chemical reaction, outlining the sequence of elementary steps leading to product formation.
- 6. A theory that explains how chemical reactions occur and why rates differ for different reactions; states that particles must collide with the correct orientation and sufficient energy to react.
- 7. A high-energy, unstable arrangement of atoms formed during a reaction, representing the point at which bonds are breaking and forming.
- 8. A proportionality constant in the rate law equation, k, which changes with temperature and determines the rate at which a reaction proceeds under given conditions.
- 11. A reaction where the rate is independent of the concentration of the reactants, meaning that changes in the reactant concentration do not affect the rate of the reaction.
- 13. A reaction where the rate is directly proportional to the concentration of one reactant, often written as Rate=k[A].
- 14. The slowest step in a reaction mechanism, which limits the overall rate of the reaction and determines the reaction rate law.
- 16. A molecular entity that forms during a multi-step reaction, which is not present in the final products but is essential for the overall reaction mechanism.
- 18. A measure of the average kinetic energy of the particles in a system; an increase in temperature generally increases the reaction rate by providing more energy for collisions.
- 20. A thermodynamic quantity that represents the degree of disorder or randomness in a system; symbolized as S, it typically increases in spontaneous processes.