**Unformatted text preview: **Rate Laws and Order of Read-10h;
Am) + 23 (aq) "> 35 (s) + 41) (aq) FirsT-Order Reactions .ﬁmv rdeovxskif U-ww . 3. \ 5+ Order Rafe (mol/L 5)
ﬁ 3 E?
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8 Q a 9 % 32 Conc. (mol/L) Second Order Reacfions .. OlUxOO‘VOVHC-I v€\oér\~0I/\Ilhf]7 \5\—\Nv\ mm \L mm :0 and
Grdlev L Conc. (mol/L) Rafe (mol/L s) RaTe Law RaTe Law- The r'aTe will always be pr'opor'Tional To The iniTial concenTr'aTion of The
r'eacTanTs ThaT are raised To some exponenTial value (deTer'mined empirically). 7‘
aA+bB-->cC+dD ’7CD
mexfl. r'aTeb<[A]“[B]" r'aTe = k[A]’“[B]n ’l .
maVeS los‘vln ﬁche; Q (1L 4e ilrs uvulS
\f\ dnom e Using The RaTe Law EquaTion Ex. 1 / K
The WT for- The r'eacTion HNQ + NH3 --> NH4N03 is 14.5 L/mol -s. If The
iniTiaI concenTraTion of niTric acid is 0.050 M and The iniTiaI concenTraTion of ammonia is 0.10 M, whaT will The r'aTe of This r'eacTion be? (r' = k [HNOS] [NH3]) =ILiSL/moi-s r: KENDQCNTQ‘ :.{WSJZ\(ODSM\(0\10\
W L,
:0 0925 moi5 L. "’ O 011 mO\/[_ 5 Ex. 2 When Two compounds, A and B, are mixed TogeTher', They form compound C, by
a r'eocTion ThoT's noT well under'sTood. ForTunoTely, The following r'oTe
infor'moTion was exper'imenTolly deTer'mined, as shown below: a) DeTer'mine The r'oTe expression for- This r'eocTion
b) DeTer'mine The r'oTe consTonT for- This r'eocTion. .3
:mo :2 E: {Cox/0 :2 ——’ 0.05 \n H .ox/(T3 l” q (Ajm a: m; l
a 0< m“ Overall Order of ReacTions The sum of The exponenTs in The raTe low expression equals The overall
order of The reacTion. .Ex. aA + bB + cC --> dD + eE P = k[""]Z[|3]1[C]0 5° Overs“ Oder {s 3. ...

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