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PORTAGE CHEM 104 MODULE
1 STUDY GUIDE
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Kinetics: the study of rates of reactions and how they are influenced by certain factors
1. Influences Reactions Rates: Concentration, temperature, catalysts, surface
area
2. Temperature/Reaction Rate: Increase, higher temperature provides higher
kinetic energy
3. Catalyst/Reaction Rate: Increase, without being consumed
4. Surface Area/Reaction Rate: Increase, increased surface area of particles
increases reaction rate because solids only react at their surfaces (grinding solid into fine powder)
5. Concentration/Reaction Rate: Increase, provides more reacting particles to
undergo reaction
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- Reaction Rate: Increase in molar concentration of product per unit of time or
the decrease in molar concentration per unit of time
7. Reaction Rate Units: moles per liter per second (mol/L*s)
8. Reaction Rate Equation: Change in concentration/change in time
(products=positive, reactants=add negative sign)
- Average Rate: Determined by using initial and final concentrations and initial
and final times so that the result measures the rate over the entire reaction
10. Instantaneous Rate: The change in concentration of reactants (or products)
divided by a very short period of time
11. Instantaneous Rate Decreases...: Decreases, as reaction proceeds,
concentration of reactant becomes smaller due to consumption of reactants as reaction takes place
12. Early Instantaneous Rate: The change in concentration of reactants (or
products) divided by a very short period of time near the beginning of the
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reaction 14. Late Instantaneous Rate: The change in concentration of
reactants (or products) divided by a very short period of time at the end of the reaction
- Relative Values of Average Rate, Early Instantaneous Rate, and Late
Instantaneous Rate: The early instantaneous rate will be greater (most
reactant) than the late instantaneous rate or the average rate. The late instantaneous rate will be smaller (less reactant) than the early instantaneous rate or the average rate.
16. Rate Law: Mathematical equation that describes the dependence of the
reaction rate on the concentrations of some of the reactants
