Question

Living organisms are highly structured, and therefore much lower in entropy than the substances from which they grow. How is it possible that these (local) entropy decreases can occur?

a) The Earth re-emits as much energy as it absorbs while keeping the same temperature, so the change in heat is zero, making the change in entropy of the Earth zero.

b) The entropy of one part of the universe can decrease provided the total entropy of the universe increases. Energy transfer is necessary for this to happen: the part of the universe with decreasing entropy cannot be isolated.

c) Plants are special: they can violate 2nd law of thermodynamics by absorbing energy coming from the Sun to decrease their entropy without increasing their temperature or increasing the entropy of anything else.

d) The 2nd law of thermodynamics is true on average, but very unlikely things can happen, and once they happen, they are likely keep on happening even in an isolated system.

Answer 1

In simple words , entropy is measure of molecular disorder or in simple words randomness of a system . It is extensive property

Its calculated on basis of Joule / Kelvin.

According to universe and earth principles , earth re-emits energy while absorbing , keeping the temperature constant , so change in internal energy is zero and since no extra work is done this corresponds to change in work done as zero . Thus change in heat therefore is zero .

Now we all know that entropy ( S ) = (heat absorbed / released ) / Temperature.

Thus entropy on account of zero heat absorbed is basically zero .

Thus this fundamental principle , i.e more structured or less randomness can always decrease the randomness.

Thus correct option would be option -A