Rate Comparisons
Related Examples and Practice Problems
Additional Worked Out Examples/ Practice
Identifying classification types: Differentiation between elements, compounds or mixtures and homogeneous and heterogenous mixtures
Separation techniques: Selected and explaining limitation of appropriate separation
Relating Properties to Composition: Predicting classification based on descriptive properties
Topic Summary & Highlights
and Help Videos
Core Concept
The rate of a reaction measures how quickly reactants are consumed or products are formed over time.
Expression: $\text{Rate} = -\frac{\Delta [\text{Reactant}]}{\Delta t} = \frac{\Delta [\text{Product}]}{\Delta t}$
where [X] is the concentration of species X and t is time.
Practice Tips
The rate of a reaction is the change in concentration of reactants or products over time, often expressed as $Rate} = \frac{\Delta[\text{Reactant}]}{\Delta t}$.
Comparing Rates of Reaction
Reaction Rate: The concept of reaction rate is fundamental in chemical kinetics. It is defined as the rate at which the concentrations of reactants decrease or the concentrations of products increase over time. This rate can be measured and expressed in terms of the change in concentration of a reactant or product per unit time, typically in units of molarity per second (M/s).
Comparing Rates of Reactions
Use stoichiometric relationships:
\text{Rate of disappearance of A} = -\frac{1}{a} \frac{\Delta [\text{A}]}{\Delta t}
\text{Rate of formation of B} = \frac{1}{b} \frac{\Delta [\text{B}]}{\Delta t}
where a and b are stoichiometric coefficients.
