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by: Ariel Kamen

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# Chemistry Week 5 Notes chem 132

Marketplace > Towson University > Chemistry > chem 132 > Chemistry Week 5 Notes
Ariel Kamen
Towson

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These are the notes that we covered this week of class.
COURSE
general chemistry lecture 2
PROF.
Sarah T. Stokes
TYPE
Class Notes
PAGES
3
WORDS
KARMA
25 ?

## Popular in Chemistry

This 3 page Class Notes was uploaded by Ariel Kamen on Thursday March 3, 2016. The Class Notes belongs to chem 132 at Towson University taught by Sarah T. Stokes in Winter 2016. Since its upload, it has received 12 views. For similar materials see general chemistry lecture 2 in Chemistry at Towson University.

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Date Created: 03/03/16
3/3/16                                      Practice 14.8  K = 3.32 x 10^­10 s^­1  at 25 degrees C. Find the rate constant at 40 degrees C. The Ea = 116  KJ/mol In(K2/K1) = Ea/R [T2 — T1/ T2 * T1] 116 KJ/mol —> 11600 J/mol *rate constant goes up by a factor of two then the rate foes up by two as well Practice 14.9     NO3 = intermediate E.S. #1 NO2 + NO2 —> NO + NO3 E.S. #2 NO3 + CO —> NO2 + CO2                   rate = K[NO2]^2                                                 *what is the rate determining step? _________________________________ NO2 + CO —> NO + CO2 rate = K[NO2]^2 (1st) rate = K[NO3][CO]^2 (2nd) rate = K[NO3]^2 <— overall C8H18 + O2 —> CO2 + H2O      catalytic converter/generally a solid Chapter 15: Equalibrium Table 15.1 Initial concentration                                                Equilibrium concentration         [NO2]      [N2O4]                                                      [NO2]            [N2O4]   0.000       0.670                                                        0.0547          0.643   0.200       0.000                                                        0.0204          0.0898 @ equilibrium [NO2]/[N2O4]                 [NO2]^2/[N2O4] 0.0881 & 0.227                 4.68x10^­3 & 4.63x10^­3 = the same N2O4 <— —> 2 NO2 K = [NO2]^2/[N2O4] aA + bB <— —> cC + dD             A + 2B <— —> AB2 K = [D]^d [C]^c / [A]^a [B]^b   rate = Kf [A][B]^2                                                rate = Kf [AB2] rate = Kf [A][B]^2 = Kf [AB2] Kf = forward ; Kr = reverse K = Kf / Kr = [AB]/[A][B]^2 N2 (g) + 3H2 (g) <— —> 2NH3 (g)      Kc = [NH3]^2 / [N2][H2]^3      Kp = P^2 NH3 / PN2 PH2^3

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