An ideal gas is confined to a cylinder by a piston. The piston is slowly pushed in so that the gas temperature remains at 20 degrees Celsius. During the compression, 730 J of work is done on the gas. Part A) Calculate the entropy change of the gas. Part B) Describe clearly why isn’t the result a violation of the entropy statement of the second law, ΔS  0 ?

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Explanation:

(a) It is given that the gas is ideal. Formula for change in entropy of the gas according to the first law of thermodynamics is as follows.

For isothermal process, at constant temperature.

So,  

or,       dQ = dW = 730 J

Now, according to the second law of thermodynamics the entropy change is as follows.

                        =

                        = 2.490 J/K

Therefore, the entropy change of the gas is 2.490 J/K.

(b)  In the given process, at constant temperature the gas will be compressed slowly because then kinetic energy of the gas molecules will also be constant. The volume decreases so that the movement of molecules increases as a result, entropy of molecules will also increase.

This means that

what are the statements?

explanation:

give me the statements and i'll tell you which is correct

a rain shadow is a dry region of land on the side that is protected against the prevailing winds of a mountain range. the prevailing winds are the winds that occur most of the time in a particular place of the earth

prevailing winds carry air toward the mountain range. as the air rises up over a mountain range, the air cools, water vapor condenses, and clouds form. on this side of the mountains, called the windward side, precipitation falls in the form of  rain  or snow. this dry air produces a  rain shadow.