Chemical Reaction Rate Flashcards

A set of vocabulary flashcards covering the fundamental concepts of chemical reaction rates, collision theory, and factors affecting reaction speed based on the lecture notes.

Reaction Rate

Measures how fast reactants become products, with examples ranging from fast reactions like fireworks to slow reactions like rusting iron.

Activation Energy

The minimum amount of energy required for a reaction to happen.

Endothermic Reaction

A reaction where energy is absorbed, resulting in the energy of products being higher than the energy of reactants.

Exothermic Reaction

A reaction where energy is released and the enthalpy change satisfies $\Delta H < 0$.

Transition state

The state representing the peak of the activation energy barrier during the reaction progress with time $(s)$.

Collision Theory

The principle that particles must collide with enough energy and correct orientation for a reaction to occur.

Temperature (Effect on Rate)

Higher temperature increases particle movement, leading to more energetic collisions and an increased reaction rate.

Concentration (Effect on Rate)

The presence of more particles in the same space, leading to more frequent collisions and faster reactions.

Surface Area (Effect on Rate)

Crushed solids react faster because more particles are exposed, allowing for more collisions to occur.

Catalyst

A substance that speeds up reactions by lowering activation energy without being consumed in the reaction.

Average Speed ($V_m$)

A measure of reaction rate calculated using the formula $V_m = \frac{\Delta [A]}{\Delta t}$.

Reaction Rate Units

The concentration change over time, expressed in the transcript as $\text{mol L}^{-1} \cdot \text{S}^{-1}$.