University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2020
Views:

372

Pages:

1
Author:

Edgar Rowe

General Chemistry 5: Chemical Kinetics m Order Rate Law Integrated Rate Law 0 zeroth order 𝑅 =𝑘 [A] = [A]@ −𝑘;𝑡 1 first order 𝑅 =𝑘;[A] [A] = [A]@ ×𝑒&A;0 2 second order 𝑅 =𝑘;[A]_ 1 1 = + 𝑘𝑡 [A] [A]@ [A] [A]@ 2;𝑘 𝑀 𝑠 ln;(2) 𝑘 1 𝑠 𝑡^ =; 𝑡^ =; 𝑡^ =; Units of Rate Constant 1 𝑀;𝑠 1 𝑘;[A]@ 1 ln;[A] Zeroth Order Reaction Half Life [A] First Order Reaction Second Order Reaction Reaction Order and Michaelis-Menten Curve: At low substrate concentrations, the reaction is approximately FIRST-ORDER. At very high substrate concentration, the reaction approximates ZERO-ORDER since the reaction ceases to depend on substrate concentration. Types of Reactions Combination: Two or more reactants forming one product. 2H2 (g) + O2 (g) 2H2O (g) Decomposition: Single reactant breaks down. 2HgO (s) 2Hg (l) + O2 (g) Combustion: Involves a fuel, usually a hydrocarbon, and O2 (g). Commonly forms CO2 and H2O. CH4 (g)+ 2O2 (g) CO2 (g) + H2 O(g) Single-Displacement: An atom or ion in a compound is replaced by another atom or ion. Cu (s) + AgNO3 (aq) Ag (s) + CuNO3 (aq) Double-Displacement: Elements from two compounds swap places. (metathesis) CaCl2 (aq)+ 2AgNO3 (aq) Ca(NO3)2 (aq) + 2AgCl(s) Neutralization: A type of double-replacement reaction. Acid + base salt + H2O HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) Hydrolysis: Using water to break the bonds in a molecule. Equations Arrhenius: 𝑘 = 𝐴×𝑒 &'( )* Definition of Rate: For aA + bB ® cC + dD Rate =− D[-] /D0 =− D[1] 2 D0 = ? Rate Law: rate=𝑘; [A] ;[ B] = D[3] 4 D0 = D[5] 6 D0 Radioactive Decay: [A]0 = [A]@ ×𝑒A0 Reaction Mechanisms Overall Reaction: A2 + 2B Step 1: Step 2: 2AB A2 + B A2B A2B + B 2AB slow fast A2B is an intermediate Slow step is the rate determining step Arrhenius Equation Arrhenius: 𝑘 = 𝐴×𝑒 Gibbs Free Energy ∆G=EO −EO;PQR −∆G=Exergonic +∆G=Endergonic &'( )* k = rate constant A = frequency factor Ea = activation energy G R = gas constant = 8.314; HIJ;K T = temp in K Trends: #A Þ #k #T Þ #k (Exponent gets closer to 0. Exponent becomes less negative)