# Chemistry 1B Kinetics

 reaction rates: the change of the concentration of the reactants and products over a given time rate orders: equation: parameter determined experimentally that relates reaction rates to concentration of the reactants rate constant (k): probability constant that relates reaction concentration to rate rate law: rate=k[A][B]2 (would be third order) an equation that defines the relationship between reaction concentration and rate equation to determine rate order for "hard case" 1st order reaction integrated rate law equation: Also, how to plot and what it would look like •plot ln(A) vs timeif 1st order:  the slope is negative (-k) and it's a straight line half life 1st order reaction equation: 2nd order reaction integrated rate law: also, how to plot and what it would look like •plot 1/A vs timeif 2nd order: the slope is positive (+k) and it's a straight line half life 2nd order reaction equation: zero order reaction equation Also, plot •plot [A] vs timeif zero order slope is negative (-k) and linear half-life zero order reaction equation: Arrhenius equation: where R=8.314 J/mol KT= temperature in KGraphic Ea determination: point method:  define catalyst increases rate of reaction without being consumed in reaction.Also, you can increase your energy in the beginning and lower your transition state energy from different, more stable complexes Authorkjel ID314992 Card SetChemistry 1B Kinetics DescriptionChemistry 1B Kinetics Updated2016-02-03T23:40:46Z Show Answers