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

Plzz a sample of table sugar (sucrose, c12h22o11) has a mass of 7.801 g. ● a) calculate the number of moles of c12h22o11 in the sample b) calculate the number of moles of each element in c12h22o11 (number of moles of c, number of moles of h & number of moles of o) in the sample. (use your answer from part a as your starting point.) show your work and highlight your final answer. calculate the number of atoms of each element in c12h22o11 (number of atoms of c, number of atoms of h & number of atoms of o) in the sample. (use your answers from part b as your starting for each element.) show your work and highlight your final answer.