Second Law of Thermodynamics: Examining the Relationship between Entropy and Spontaneous Processes.

For each of the following processes, predict whether the entropy of the universe increases or decreases.

Entropy increases: C6H12O6(s)+6O2(g)→6CO2(g)+6H2O(l)Formation of a bilayer after lipids are mixed with an aqueous solutionEntropy Decreases: The original mixing of oil and water, before it separates3H2(g)+2N2(g)→2NH3(g)

1) Combining hydrogen and oxygen to form water

The entropy of the universe increases in this process because the reactants (hydrogen and oxygen) have fewer energetically equivalent ways of arranging themselves compared to the products (water molecules).

2) Melting a block of ice

The entropy of the universe increases in this process because the solid ice has a more ordered structure and lower entropy than the liquid water.

3) Dissolving salt in water

The entropy of the universe increases in this process because the salt ions become more dispersed and randomized in the water, creating more energetically equivalent arrangements.

4) Heating up a metal rod

The entropy of the universe increases in this process because the increased temperature of the metal rod causes more random and varied vibrations of its atoms, increasing disorder.

Overall, the second law of thermodynamics states that the entropy of the universe always increases in any spontaneous process, where entropy is a measure of the degree of randomness or disorder in a system.

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