CHM135H1 Chapter Notes - Chapter 13: Reaction Step, Reaction Intermediate, Reaction Rate

• School: UTSG
• Department: Chemistry
• Course: CHM135H1
• Professor: Kris Quinlan

Document Summary

Kinetics: (how: explains how reactions take place, how quickly it occurs. Rate of reaction: measured in changes of concentration per unit time (ms-1 or mol/ls, slows down within time, look at coefficients to see how much increases/decreases, 2no2cl 2no2 + cl2. For every mol of no2cl, one mol of no2 is produced, while mol of cl2 is produced. Integrated rate law: concentration-time equations that allows us to calculate the concentration of reactant that remain at any t within a reaction, zeroth-order reactions: (slope = -k) (units: m/s or m-1s-1) *we graph [a] vs time; if the graph has a linear slope then the reaction is zeroth order. (integrated for zeroth order reaction: first-order reactions: (slope = -k) (units: 1/s or s-1) (integrated for first order reaction) . 89: (half-life is constant for first order reactions) *we graph ln[a] vs time; if the graph has a linear slope then the reaction is first order: second-order reactions: (slope = k)