Midterm 08

# Midterm 08 - DATA THAT YOU MAY USE Units Volume Pressure...

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DATA THAT YOU MAY USE Units Conventional S.I. Volume mL or cm 3 = cm 3 or 10 -3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = 1.013 × 10 5 Pa torr = 133.3 Pa Temperature ° C 0 ° C = 273.15 K PV L-atm = 1.013 × 10 5 dm 3 Pa =101.3 dm 3 kPa =101.3 J Energy 1 cal = 4.184 J (J= kg m 2 /s 2 ) 1 erg = 1 g cm 2 /s 2 = 10 -7 J Current ampere (A) = 1 C/s Constants Avogadro’s number N 6.022 × 10 23 mol -1 Boltzmann’s constant k 1.381 × 10 -23 J K -1 Faraday’s constant F 96 485 C mol -1 Values of R for various unit combinations 1.986 cal mol -1 K -1 0.08206 L atm mol -1 K -1 82.06 cm 3 atm mol -1 K -1 8.314 J mol -1 K -1 8.314 × 10 7 erg mol -1 K -1 8.314 dm 3 kPa mol -1 K -1 8.314 × 10 3 cm 3 kPa mol -1 K -1 Clausius-Clapeyron Equation Quadratic Formula = 2 1 1 2 1 1 ln T T R H P P vap a ac b b x c bx ax 2 4 0 2 2 ± = = + +

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Integrated Rate Laws Arrhenius Equation Order 0: [A] = [A] 0 k t / a E RT k Ae = Order 1: [A] = [A] 0 e - k t 2 1 21 11 ln a E k k RTT  =   Order 2: 1/[A] = 1/[A] 0 + kt Δ G (non-standard conditions) van ‘t Hoff Equation Δ G = Δ + RT ln Q 2 1 ln o K H K R TT −∆ = Gas Laws nRT PV = 2 2 2 2 1 1 1 1 T n V P T n V P = RT MP d = RT MPV m = 2 3 1 u m V N P = A k N RT e 2 3 = M RT u rms 3 = hdg P = Solutions iMRT = π C=kP gas P A = χ A P A ° Common Strong Acids Common Strong Bases HCl LiOH Ca(OH) 2 HBr NaOH Sr(OH) 2 HI KOH Ba(OH) 2 HClO 4 RbOH HNO 3 CsOH H 2 SO 4 Mg(OH) 2
The Periodic Table of the Elements

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1) A 10 L container holds a mixture of 5 gases at 0ºC. The composition of the mixture is given below. What is the partial pressure of N 2 ? N 2 (g) 10 g O 2 (g) 1 g H 2 (g) 20 g CO 2 (g) 7 g He (g) 3 g a) 608 torr b) 800 torr c) 1340 torr d) 932 torr e) 22 torr 2) If a liter of argon gas (Ar) is compared to a liter of neon gas (Ne), both at 75°C and two atmospheres of pressure, then: a) There are equal numbers of Ar and Ne atoms. b) The Ar and Ne atoms have the same average speed. c) The Ne atoms are on the average moving more slowly than the Ar atoms.
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## This note was uploaded on 04/20/2011 for the course CHEM 120 taught by Professor Barret during the Fall '08 term at McGill.

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Midterm 08 - DATA THAT YOU MAY USE Units Volume Pressure...

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