![]() However, if the reaction occurs at high temperature the reaction becomes nonspontaneous, for the free energy change becomes positive when the high temperature is multiplied with a negative entropy as the enthalpy is not as large as the product. When the reaction occurs at a low temperature the free energy change is also negative, which means the reaction is spontaneous. The temperature would also determine the spontaneous nature of a reaction if both enthalpy and entropy were positive. Because both enthalpy and entropy are negative, the spontaneous nature varies with the temperature of the reaction. Using the entropy of formation data and the enthalpy of formation data, one can determine that the entropy of the reaction is -42.1 J/K and the enthalpy is -41.2 kJ. Now one must find if the entropy is greater than zero to answer the question. ![]() If the enthalpy is negative then the reaction is exothermic. And one place you always find entropy is in the Second Law of Thermodynamics, because it allows us a third way to state the second law, which is that the total. The Clausius form of the second law states that spontaneous change for an irreversible process in an isolated system (that is, one that does not exchange heat or work with its surroundings) always proceeds in the direction of increasing entropy. ![]() ![]() One may have to calculate the enthalpy of the reaction, but in this case it is given. \): Matrix of Conditions Dictating Spontaneity Case
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