CHEM 110 - ° f(reactants ∆ H ° rxn = Σ n(D of bonds broken – Σ m(D of bonds formed Solubility Guidelines The following form soluble ionic

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CHEM 110 EQUATIONS Constants, conversions and equations available during exams Conversions 1 J = 1 kg · m 2 · s 2 1 cal = 4.184 J 1 atm = 760 mmHg = 760 torr 1 atm = 1.01325 × 10 5 Pa 1 atm = 101.325 kPa 1 D = 3.33 × 10 30 C · m 1 mol of gas at STP occupies V = 22.41 L Equations Constants c = 3.00 × 10 8 m · s 1 h = 6.63 × 10 34 J · s R H = 2.18 × 10 18 J N A = 6.022 × 10 23 mol 1 e = 1.60 × 10 19 C k L = 8.99 × 10 9 N · m 2 · C 2 m e = 9.109 × 10 28 g R = 8.314 J/(mol · K) R = 0.08206 L · atm/(mol · K) R = 1.987 cal/(mol · K) E = h ν λ = h/mv c = λν E k = ½ mv 2 " E = R H 1 n i 2 # 1 n f 2 $ % ' ( ) ) E = k L Q 1 Q 2 /d μ = Q r q = m · C · T d = PM/(RT) P i = X i P tot u = 3 RT M r 1 r 2 = M 2 M 1 P A = X A P A o (P + n 2 a/V 2 )(V – nb) = nRT T f = K f m T b = K b m C g = k H P g π = (n/V)RT K p = K c (RT) Δ n H ° rxn = Σ n f (products) – Σ m H
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Unformatted text preview: ° f (reactants) ∆ H ° rxn = Σ n (D of bonds broken) – Σ m (D of bonds formed) Solubility Guidelines The following form soluble ionic compounds Exceptions NH 4 + , Li + , Na + , K + , Rb + , Cs + No exceptions NO 3 − , ClO 4 − , and CH 3 COO − No exceptions Cl − , Br − , I − Ag + , Hg 2 2+ , Pb 2+ SO 4 2 − Ca 2+ , Sr 2+ , Ba 2+ , Hg 2 2+ , Pb 2+ , Ag + The following form insoluble salts Exceptions CO 3 2 − and PO 4 3 − NH 4 + , Li + , Na + , K + , Rb + , Cs + (see above) OH − and S 2 − Ca 2+ , Sr 2+ , Ba 2+ , and NH 4 + , Li + , Na + , K + , Rb + , Cs + (see above)...
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This note was uploaded on 01/18/2012 for the course CHEM 110 taught by Professor Hofmann,brucerob during the Fall '08 term at Pennsylvania State University, University Park.

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