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Chapter 5: Q. 5.3 (page 155)

Use the data at the back of this book to verify the values of ΔH and ΔGquoted above for the lead-acid reaction 5.13.

At temp 298K and pressure 1 bar.

Short Answer

Expert verified

The value of Gibbs free energy = -315.72 kJ.

Step by step solution

01

Given information

The table is given as below

Temp = 298k and pressure =1 bar

02

Explanation

Gibbs energy is given by

G = H - TS

where G= Gibbs energy, H= Enthalpy, T =temp and S =entropy.

Assume there is infinitesimal change in Gibbs energy , then

ΔG = ΔH - TΔS ..........................................(1)

Now write equation for change in enthalpy for the given reaction

ΔH=2ΔHPbSO4+2ΔHH2O-ΔHPb-ΔHPbO2+4ΔHH+-2ΔHSO42-

Substitute the values from given table we get,
ΔH=2(-920.0kJ)+2(-285.83kJ)-0-(-277.4kJ)-4(0)-2(-909.27kJ)=-315.72kJ

Similarly write equation for change in Gibbs energy for the given reaction
Put the values from the table, we get

∆G=2(-813.0kJ)+2(-237.13kJ)-0-(-217.33kJ)-4(0)-2(-744.53kJ)∆G=-315.72kJ

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Most popular questions from this chapter

Calcium carbonate, CaCO3, has two common crystalline forms, calcite and aragonite. Thermodynamic data for these phases can be found at the back of this book.

(a) Which is stable at earth's surface, calcite or aragonite?

(b) Calculate the pressure (still at room temperature) at which the other phase

should become stable.

Consider a fuel cell that uses methane ("natural gas") as fuel. The reaction is

CH4+2O2⟶2H2O+CO2

(a) Use the data at the back of this book to determine the values of ΔHand ΔGfor this reaction, for one mole of methane. Assume that the reaction takes place at room temperature and atmospheric pressure.

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(c) How much waste heat is produced, for each mole of methane fuel?

(d) The steps of this reaction are

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