AP Chemistry Chpt 12: Kinetics Flashcards
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| 1919775329 | units for k are M * s⁻¹ | zero order rxn | 0 | |
| 1919775330 | [A] = -kt + [A]₀ | integrated rate law for zero order rxn | 1 | |
| 1919775331 | [A] vs. time straight line plot | zero order rxn | 2 | |
| 1919775332 | t₁/₂ = [A]₀/2k | half life for zero order rxn | 3 | |
| 1919775333 | units for k in s⁻¹ (1/s) | 1st order rxn | 4 | |
| 1919775334 | ln[A] = -kt + ln[A]₀ | integrated rate law for 1st order rxn | 5 | |
| 1919775335 | ln[A] vs. time Straight Plot | 1st order rxn | 6 | |
| 1919775336 | t₁/₂ = ln 2/k | half life for 1st order rxn | 7 | |
| 1919775337 | units for k in M ⁻¹ * s⁻¹ | 2nd order rxn | 8 | |
| 1919775338 | 1/[A] = kt + 1/[A]₀ | integrated rate law for 2nd order rxn | 9 | |
| 1919775339 | 1/[A] vs. time Straight Plot | 2nd order rxn | 10 | |
| 1919775340 | t₁/₂ = 1/k[A]₀ | half life for 2nd order rxn | 11 | |
| 1919775341 | Activation Energy | the kinetic energy that reactant molecules must have to so that a reaction can occur. | 12 | |
| 1919775342 | Arrhenius Equation | An equation that relates the specific rate constant to activation energy and temperature. | 13 | |
| 1919775343 | Catalyst | A substance that increases the rate at which a reaction occurs. It remains unchanged when the reaction is complete. | 14 | |
| 1919775344 | Collision Theory | A theory of reaction rates that states that effective collisions between reactant molecules must take place for reaction to occur. | 15 | |
| 1919775345 | Effective Collision | A collision between molecules that results in reaction; one in which molecules collide with proper orientations and with sufficient energy to react. | 16 | |
| 1919775346 | Elementary Step | An individual step in the mechanism by which a reaction occurs. The reaction order for this step matches the reactant coefficients. | 17 | |
| 1919775347 | Enzyme | A protein that acts as a catalyst in a biological system. | 18 | |
| 1919775348 | Half-life of a Reactant | The time required for half of that reactant to be converted into product(s). | 19 | |
| 1919775349 | Integrated Rate Equation | An equation that relates the concentration of a reactant remaining to the time elapsed; has different mathematical forms for different orders of reaction. | 20 | |
| 1919775350 | Method of Initial Rates | A method of determining the rate-law expression by carrying out a reaction with different initial concentrations and analyzing the resulting changes in initial rates. | 21 | |
| 1919775352 | Rate Constant | rate=k[A]^x[B]^y. An experimentally-determined constant that is different for different reactions and that, for a given reaction, changes only with temperature or the presence of a catalyst; "k" in the rate-law expression, | 22 | |
| 1919775353 | Rate- determining Step | The slowest elementary step in a reaction mechanism; the step that limits the overall rate of reaction. | 23 | |
| 1919775354 | Rate Law | An equation that relates the rate of a reaction to the concentrations of the reactants and the specific rate constant; rate=k[A]^x[B]^y. Must be determined from experimental data. | 24 | |
| 1919775355 | Rate of Reaction | The change in concentration of a reactant or product per unit of time. (units are M / s ) | 25 | |
| 1919775356 | Intermediate | A species that is produced and then entirely consumed during a multistep reaction; usually short-lived. | 26 | |
| 1919775357 | Reaction Mechanism | The sequence of fundamental steps by which reactants are converted into products. | 27 | |
| 1919775358 | Thermodynamically favorable, spontaneous reaction | A reaction that occurs with a net release of free energy, G; a reaction for which deltaG is negative. | 28 | |
| 1919775359 | Transition state | A relatively high-energy state in which bonds in reactant molecules are partially broken and new ones are partially formed. | 29 | |
| 1919775360 | Transition State Theory | A theory of reaction rates that states that reactants pass through high-energy transition states before forming products. | 30 |