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Chapter 5: 5.3 (page 155)

Use the data at the back of this book to verify the values of ∆Hand ∆G quoted above for the lead-acid reaction 5.13.

Short Answer

Expert verified

The value of Gibbs free energy = -315.72 kJ.

Step by step solution

01

Given Information

T= 298 K and P=1 bar.

The information from the table

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

∆G=∆H-T∆S.............(1)

Now write equation for change in enthalpy for the given reaction

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

Now substitute the values from the 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

ΔG=(2ΔGPbSO4+2ΔGH2O-ΔGPb-ΔGPbO2+4ΔGH+-2ΔGSO42-)

Put the values from the table, we get

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

= -315.72 kJ.

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