Consider a process in which 1.00 mil h2o(l) at -5.0 celsius solidifies to ice at the same temperature. calculate the change in entropy of the sample, of the surroundings and the total change in entropy. is the prices spontaneous? repeat the calculations for a process in which 1.00 mol h2o(l) vaporizes at 95 celsius and 1.00 atm.

data given: cpm h20(s) 37.6j/(k* h20(l) 75.3j/(k* h20(g) 33.6—-standard enthalpy of vap and fusion are 40.7 and 6.01 kj/mol respectively