In a certain chemical reaction at standard conditions (P 1 atm, T 298 K), a lite

Question

In a certain chemical reaction at standard conditions (P 1 atm, T 298 K), a liter of Boglium reacting with half a liter of Coblium shrinks to a quarter liter of the compound Glopslop. The energy released in this reaction is used to charge a cell phone, and that energy is 160 J greater than the change in the internal chemical energy of these substances. Where did this extra energy come from? If this process is reversible, what was the total change in entropy of these substances? How much heat was either released to or absorbed by the environment, and why?

Explanation / Answer

Since the volume of the system is changing at the standard conditions, the amount of extra 160 J released due to system is due to volume shrinkage or more chemically, due to ordered arrangement of the molecules.

Now,

in a reversible process, change in total entropy of universe = 0.

Here, system is releasing energy = -160 J.

Therefore,

change in entropy of system = -160 J/mol/ 298 K = -0.54 J/mol- K

Since system is releasing energy, hence energy absorbed by surrounding or environment = 160 J.

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