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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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