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Tutorial section 1

Tutorial section 1. Numerical problems 7.6:

camilla-norton
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Tutorial section 1

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  1. Tutorial section 1

  2. Numerical problems 7.6: Calculate the equilibrium constant of the reaction CO(g) + H2(g)↔ H2CO(g) given that, for the production of liquid formaldehyde, ΔrGθ= 28.95 kJ mol-1 at 298 K and that the vapour pressure of formaldehyde is 1500 Torr at that temperature.

  3. Numerical problem 7.7 Acetic acid was evaporated in container of volume 21.45 cm3 at 437 K and at an external pressure of 101.9 kPa, and the container was then sealed. The mass of acid present in the sealed container was 0.0519 g. The experiment was repeated with the same container but at 471 K, and it was found that 0.0380 g of acetic acid was present. Calculate the equilibrium constant for the dimerization of the acid in the vapour and the enthalpy of vaporization. (there is a typo in the solution manual (1+alpha)n

  4. Numerical problem 7.8 A sealed container was filled with 0.300 mol H2(g), 0.400 mol I2(g), and 0.200 mol HI(g) at 870 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 870 for the reaction H2(g) + I2(g) ↔ 2HI(g).

  5. Numerical problem 7.16 Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg-1)|Hg2Cl2(s)Hg(l), for which the cell reaction is Hg2Cl2(s) + Zn(s) →2Hg(l) +2Cl-(aq) + Zn2+(aq). Given that Eθ(Zn2+,Zn) = -0.7268 V, Eθ(Hg2Cl2,Hg) = 0.2676 V, and that the emf is 1.2272 V, (a) write the Nernst equation for the cell. Determine (b) the standard emf, (c) ΔrG, ΔrGθ, and K for the cell reaction, (d) the mean activity and activity coefficient of ZnCl2 from the measured cell potential, (e) the mean ionic activity coefficient of ZnCl2 from the Debye-Huckel limiting law, (f) Given that (∂E/∂T)p = -4.52 x 10-4 V K-1. Calculate ΔS and ΔH.

  6. Numerical problem 7.20 The standard potential of the AgCl/Ag,Cl- couple has been measured very carefully over a range of temperature and the results were found to fit the expression Eθ/V = 0.23659 – 4.8564x10-4(θ/oC) – 3.4205 x 10-6(θ/oC)2 + 5.869x 10-9(θ/oC)3 Calculate the standard Gibbs energy and enthalpy of formation of Cl-(aq) and its entropy at 298 K.

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