Entropy Exploration In which direction do chemical svstems become more disordere

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Entropy Exploration In which direction do chemical svstems become more disordered? From the class examples, we came to the conclusion that naturally occurring processes tend to move toward a state of greater disorder. We know that dissolving contaminants into silicon is a spontaneous process, and that the process increases disorder. Knowing whether a reaction causes more order or disorder is crucial in deciding whether a reaction will happen (1) under certain conditions and (2) at all. However, it is not always easy to decide whether one state is more disordered than another. We would like to be able to compare relative "amounts" of order in chemical systems. The goal of these questions is to answer the question: In which direction do chemical sstems become more disordered? You already know that dissolving and mixing are processes that can occur without the transfer of significant amounts of heat and work. They are often spontaneous because they tend to increase the disorder of a system. What about other types of processes? How do they change disorder of a svstem? the The disorder that we have been discussing has another name: entropy (S), defined as the degree of randomness of a system. Entropy leads us to a definition of the Second Law of Thermodynamics: whenever a spontaneous change takes place in our universe, it is accompanied by an overall increase in entropy. Like the First Law of Thermodynamics, the Second Law has not been proven; however, it has never been disproved. A mathematical way to state the Second Law of Thermodynamics is ASuniverse ASsystem+ ASsurroundings >0 In a spontaneous process, the entropy or disorder of the universe increases. The total disorder of the universe can arbitrarily be divided into the disorder of the system and the disorder of the surroundings (i.e., everything else). Notice that the entropy of the system can decrease if the entropy of the surroundings increases, and vice versa. In chemistry, we are primarily concerned with the entropy changes of chemical systems, not the surroundings or the universe. While the Second Law always predicts spontaneity, it is difficult to keep track of the order in the entire universe! How do we know when the entropy of a system is increasing? Here are a few guidelines

Explanation / Answer

1. a) ?S is +ve(solid is converting in to gas plus solid products. spontaneous reaction)

b) ?S is +ve(solid is converting in to solid plus gas products. spontaneous reaction)

c) ?S is -ve ( gas is converting in to solid. Non spontaneous reaction)

D) ?S is -ve ( liquid plus solid converting in to solid. Non spontaneous reaction.)

E) ?S is +ve ( solid is absorbing heat so molecules can randomly move in all directions which results in increase in entropy)

2. For the reaction ?S greater than zero, the reaction should be endothermic. So entropy will increase i.e. disorderness of molecules increases.

3. For the reaction e entropy change is charge. Because reaction absorbed more heat.

4. Yes. Different gases will mix together as much as they can. Resulting in increase of entropy( randomness increases)

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