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Midterm

Midterm 08.pdf

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Department
Chemistry
Course
CHEM 110
Professor
Sebastien Breau
Semester
Fall

Description
DATA THAT YOU MAY USE Units Conventional S.I. 3 3 -3 3 Volume mL or cm = cm3or 10 dm Liter (L) = dm Pressure atm = 760 torr = 1.013 × 10 Pa torr = 133.3 Pa Temperature °C 0°C = 273.15 K PV L-atm = 1.013 × 10 dm Pa 3 =101.3 dm kPa =101.3 J Energy 1 cal = 4.184 J (J= kg •m /s ) 2 2 -7 1 erg = 1 g cm/s = 10 J Current ampere (A) = 1 C/s Constants Avogadro’s number N 6.022 × 10 mol-1 -23 -1 Boltzmann’s constant k 1.381 × 10 J K -1 Faraday’s constant F 96 485 C mol Values of R for various unit combinations -1 -1 1.986 cal mol K 0.08206 L atm mol K-1 82.06 cm atm mol K -1 -1 -1 8.314 J mol K 8.314 × 10 erg mol K-1 8.314 dm kPa mol K -1 3 3 -1 -1 8.314 × 10 cm kPa mol K Clausius-Clapeyron Equation Quadratic Formula 2 ax b+ + =  P  ∆ H  1 1  ln 2 = vap  −  2     − ± b − 4ac  P 1 R  T1 T2  x= 2a Integrated Rate Laws Arrhenius Equation Order 0: [A] = [A] t k = Ae −Ea/RT 0 k −E 11 ln 2 = a  − Order 1: [A] =0[A] t k RT T 1 2 Order 2: 1/[A] = 1/[A] 0 ΔG (non-standard conditions) van ‘t Hoff Equation K2 −∆ H o 11 ΔG = ΔG° + RT ln Q ln =  − K1 R TT 2 1 Gas Laws P1 1 P2 2 MP MPV PV = nRT = d = m = n1 1 n2 2 RT RT 1 N 3 RT 3RT P = mu 2 ek= u = P = hdg 3 V 2 N A rms M Solutions π=iMRT C=kPgasAχ AA° Common Strong Acids Common Strong Bases HCl LiOH Ca(OH)2 HBr NaOH Sr(OH2 HI KOH Ba(OH)2 HClO RbOH 4 HNO 3 CsOH H2SO4 Mg(OH)2 The Periodic Table of the Elements 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 2g) 10 g O 2g) 1 g H 2g) 20 g CO (2) 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. d) The mass of one liter of Ar equals the mass of one liter of Ne. e) The average kinetic energy of the Ar atoms isgreater than that of the Ne atoms. 3) Which gaseous mixture contains the largest number of moles of oxygen (O 2)? a) 1 L of gaseous mixture at 0ºC with an O 2partial pressure of 500 torr and a N 2artial pressure of 4000 torr b) 20 L of gaseous mixture at STP containing 50% O by vo2ume c) A gaseous mixture of 150 g of O and225 g N in a 20 L container d) 0.5 moles of O and 3 moles of N in a 10 L container 2 2 e) 50 L of a gaseous mixture at STP with an O mole2fraction (χ ) of O21. 4) Calculate u , in m/s, for H (g) molecules at 30°C. rm3 2 a) 5.26 × 10 2m/s b) 6.09 × 10 m/s c) 6.13 × 10 1m/s 3 d) 2.74 × 10 m3s e) 1.94 × 10 m/s 5) Complete this sentence: The molecules of different samples of an ideal gas have the same average kinetic energies, at the same ________. a) pressure b) temperature c) volume d) density e) molarity 6) For the reaction: Kp= 6.4 × 10 -6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227 °C such that [C2 ] = 0.5 M, [2 O] = 0.40 M, [HCl] = 0.5 M, and [O 2 = 0.015 M, in which direction will the reaction proceed? a) The reaction proceeds to the left. b) The reaction volume must be specified to answer this question. c) The value of K pt 25 °C must be specified to answer this question. d) The reaction proceeds to the right. e) The reaction is already at equilibrium. 7) Considering that the following reaction is exothermic, choose the correct statement: a) The reaction will be spontaneous at
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