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Tutorial Section 1

This document contains instructions and descriptions for solving several numerical chemistry problems involving thermodynamic calculations: 1) Calculating the equilibrium constant for the reaction CO(g) + H2(g) ↔ H2CO(g) given standard Gibbs free energy and vapor pressure data. 2) Calculating the equilibrium constant and enthalpy of vaporization for the dimerization of acetic acid in the vapor phase using experimental data on vapor pressures. 3) Calculating component amounts at equilibrium for a reaction of H2(g), I2(g), and HI(g) given an equilibrium constant. 4) Using thermodynamic data to determine standard Gibbs free energy, entropy, and

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195 views6 pages

Tutorial Section 1

This document contains instructions and descriptions for solving several numerical chemistry problems involving thermodynamic calculations: 1) Calculating the equilibrium constant for the reaction CO(g) + H2(g) ↔ H2CO(g) given standard Gibbs free energy and vapor pressure data. 2) Calculating the equilibrium constant and enthalpy of vaporization for the dimerization of acetic acid in the vapor phase using experimental data on vapor pressures. 3) Calculating component amounts at equilibrium for a reaction of H2(g), I2(g), and HI(g) given an equilibrium constant. 4) Using thermodynamic data to determine standard Gibbs free energy, entropy, and

Uploaded by

crazy
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Tutorial section 1

• 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.
• 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


• 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).
• 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.
• 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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