Practice Problem 8

Predict whether the following reaction is still spontaneous at 500C:

N2(g) + 3 H2(g) equilibr.gif (63 bytes) 2 NH3(g)

Assume that the values of  deltaHo and deltaS used in Practice Problem 7 are still valid at this temperature.


Before we can decide whether the reaction is still spontaneous we need to calculate the temperature of the kelvin scale:

TK = 500o C + 273 = 773 K

We then multiply the entropy term by this temperature and subtract this quantity from the enthalpy term:

deltaGo773 = deltaHo298 - T deltaSo298

            = 92,220 J - (773 K x -198.75 J/K)

        = 92,220 J - (-153,600 J)

        = 61,380 J

deltaGo = 61.4 kJ

Because the entropy term becomes larger as the temperature increases, the reaction changes from one which is favorable at low temperatures to one that is unfavorable at high temperatures.

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