A) Suppose you dump a bucket of water (5.00kg at 15.0C) outsideon a cold night where T = -10.0C, and the water spreads out over anarea so large that the temperature of the ground remains at -10.0C,acting like an ideal “cold reservoir.” Calculate the entropy changeof the water in going from 15.0C to -10.0C, and calculate theentropy change of the environment, absorbing heat while staying(approximately) at -10.0C. This problem requires you to use TWOequations for entropy change – of a substance changing temperatureand for a substance with Q in or out but at constant T. I gotsomewhat less than 8000J/K for the “environment’s” ∆S.

B) Use your answers to part A to solve for the total entropychange of the UNIVERSE in that process (ie, add the entropy changesof all the parts, confirming that the entropy change of theUNIVERSE is positive.)

C) Some people uncomfortable with the idea of evolution try toargue against it because, they say, it says that more “ordered”organisms evolve from less ordered organisms. Since entropy is ameasure of “disorder,” this can’t happen. Now suppose for a momentthat if you really did calculate the entropy of a bunch of“biomass” of 1 billion years ago, full of primitive organisms and afew inorganic compounds, and the equivalent “biomass” of a fewpeople, and you found that the entropy WAS lower for the people,indicating that, yes indeed, the more complex organisms DO havelower entropy than the equivalent “primitive stuff” of which theywere made. Why does this STILL not violate the second law ofthermodynamics? (Hint: is part B fundamentally different from partA of this exercise, or are they fundamentally the same?)