Question

Consider the following equation. Fe2O3(s) 3H2(g) Right arrow. 2Fe(s) 3H2O(g) Delta. H = 98. 8 kJ, and Delta. S = 141. 5 J/K. Is this reaction spontaneous or nonspontaneous at high and low temperatures? spontaneous at high temperatures, nonspontaneous at low temperatures nonspontaneous at high and low temperatures spontaneous at low temperatures, nonspontaneous at high temperatures spontaneous at high and low temperatures.

Answer 1

The reaction is spontaneous at high temperatures, and non-spontaneous at low temperatures.

In a thermodynamically closed system, the measure of the non-expansion work by the system and the enthalpy and the entropy is said to be the Gibbs free energy.

How to determine the Gibbs free energy?

According to the reaction, the enthalpy change $(\rm \Delta H)$ and the change in the entropy $(\rm \Delta S)$ is positive. The Gibbs free energy is given by, $\rm \Delta G = \Delta H - T \Delta S$ and the reaction will be spontaneous only when the $\rm\Delta G$ is negative.

If there is not much effect on the enthalpy and entropy due to a decrease in temperature, then the value of the Gibbs free energy will be positive and will be close to that of the enthalpy change. In the above reaction enthalpy, change is positive and hence the reaction will be non-spontaneous.

When the temperature is increased then the entropy will affect the overall reaction as the Gibbs free energy will have the opposite sign as that of the entropy. So the reaction will become spontaneous at high temperatures.

Thus, option A is correct.

Learn more about Gibbs free energy here:

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