CHEM-C 117 Study Guide - Midterm Guide: Molecularity, Reaction Rate, Nitrogen Dioxide
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As reaction progresses, number of molecules of reactants go down, products go up. Rate law- shows how the rate depends on the concentrations of reactants. Cannot be written from balanced equation change in rate is based solely on one reactant: ex. Must ha(cid:448)e se(cid:448)eral trials (cid:449)here one reactant"s concentration changes and other(cid:894)s(cid:895) do not, so. Instantaneous rate- value of the rate of reaction at a particular time. Can be obtained by computing the slope of a line tangent to the curve at that point (cid:1827)= reactant: (cid:1870)(cid:1872)= [(cid:3002)] (cid:3047, (cid:1870)(cid:1872)= [(cid:3003)] (cid:3047) (cid:1828)= product, (cid:1870)(cid:1872) (cid:4672)(cid:3046)(cid:4673)=(cid:1863)[(cid:1827)](cid:3041)[(cid:1828)](cid:3040) . (cid:1866),(cid:1865)= order of the individual reactant- power to which change in concentration affects rate. Value of exponent (cid:1866) must be determined by experiment; [(cid:1832)(cid:2870)] doubles with [(cid:1829)(cid:1864)(cid:1841)(cid:2870)] constant; rate also doubles, order of (cid:1832)(cid:2870)=(cid:883) [(cid:1829)(cid:1864)(cid:1841)(cid:2870)] quadruples with [(cid:1832)(cid:2870)] constant; rate also quadruples, order of (cid:1829)(cid:1864)(cid:1841)(cid:2870)=(cid:883) [(cid:1845)(cid:2870)(cid:1841)(cid:2876) (cid:2870)] constant, [ ] halves; rate also halves, order of [ ]=(cid:883)
