| Question | Answer |
| overall reaction order | Sum of m and n |
| initial rate | Is the instantaneous rate determined just after the reaction begins |
| methods of initial rates | Experimentally determining the form of the rate law. The idea is the determine the instantaneous rate before the initial concentrations of reactants have changed significantly |
| first order | Concentration to the first power. Increases in concentration in 1:1 ratio with increase in rate. Rate = k[A] |
| Determining the form of a rate law | Determining experimentally the power to which each reactant concentration must be raised in the rate law |
| integrated rate law | Expresses how the concentrations depend on time |
| differential rate law | Tells us exactly how the rate depends on concentration of the reactant. Usually just called a Rate Law |
| order | n. Can be an integer or fraction |
| rate constant | k. Proportionality constant |
| Rate law | Shows how the rate depends on the concentrations of reactants. Rate = k[NO2]^n. Concentrations of products do not appear in rate laws because the reaction rate is being studied under conditions where the reverse reaction does not contribute to the overall rate. Value of exponent n must be determined by experiment, cannot be written from the balanced equation |
| Reversible chemical reactions | So technically rate of reaction depends on difference in rates of the forward and reverse reactions. Avoided because we usually study rate of reaction under conditions where reverse reaction negligible, so only concentrations of reactants matters |
| How do coefficients effect rate of products | In balanced equation, products with lower coefficients will be produced slower than other products |
| Instantaneous Rate | Obtained by taking the derivative at a point |
| [ ] | Square brackets indicate concentration in mol/L |
| reaction rate | Change in concentration of a reactant or product per unit time. ∆[A] / ∆t. Negative with reactant (decreasing). Positive with product (increasing). Typically not constant, mostly change with time because concentrations change |
| Reaction mechanism | Understand the steps by which a reaction takes place. Can find way to facilitate the reaction |
| Chemical kinetics | Area of chemistry that concerns reaction rates |
17 cards - created jan 7, 2:24pm