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Chapter 5: 5.3 (page 155)

Use the data at the back of this book to verify the values of 鈭�Hand 鈭�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

鈭�G=鈭�H-T鈭�S.............(1)

Now write equation for change in enthalpy for the given reaction

螖H=2螖HPbSO4+2螖HH2O-螖HPb-螖HPbO2+4螖HH+-2螖HSO42-

Now substitute the values from the given table, we get

螖H=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

螖G=(2螖GPbSO4+2螖GH2O-螖GPb-螖GPbO2+4螖GH+-2螖GSO42-)

Put the values from the table, we get

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

= -315.72 kJ.

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Most popular questions from this chapter

As you can see from Figure5.20,5.20,the critical point is the unique point on the original van der Walls isotherms (before the Maxwell construction) where both the first and second derivatives ofPPwith respect toVV(at fixedTT) are zero. Use this fact to show that

Vc=3Nb, Pc =127ab2 and kTc=827ab

Write down the equilibrium condition for each of the following reactions:

(a)2H鈫�H2(b)2CO+O2鈫�2CO2(c)CH4+2O2鈫�2H2O+CO2(d)H2SO4鈫�2H++SO42-(e)2p+2n鈫�He4

A muscle can be thought of as a fuel cell, producing work from the metabolism of glucose:

C6H12O6+6O2鉄�6CO2+6H2O

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

(b) What is maximum amount of work that a muscle can perform , for each mole of glucose consumed, assuming ideal operation?

(c) Still assuming ideal operation, how much heat is absorbed or expelled by the chemicals during the metabolism of a mole of glucose?

(d) Use the concept of entropy to explain why the heat flows in the direction it does?

(e) How would your answers to parts (a) and (b) change, if the operation of the muscle is not ideal?

Use the result of the previous problem and the approximate values of a and b to find the value of Tc, Pc, Vc/N for N2, H2O and He.

Suppose that a hydrogen fuel cell, as described in the text, is to be operated at 75掳Cand atmospheric pressure. We wish to estimate the maximum electrical work done by the cell, using only the room temperature data at the back of this book. It is convenient to first establish a zero-point for each of the three substances, H2,O2,andH2O. Let us take Gfor both H2andO2to be zero at 25掳C, so that G for a mole of H2Ois -237KJat 25掳C.

(a) Using these conventions, estimate the Gibbs free energy of a mole of H2at 75掳C. Repeat for O2andH2O.

(b) Using the results of part (a), calculate the maximum electrical work done by the cell at 75掳C, for one mole of hydrogen fuel. Compare to the ideal performance of the cell at25掳C.
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