1. The problem statement, all variables and given/known data Suppose that 1 kg of water, initially at 350 K, is turned into steam at 373 K. What is the change in entropy? (Lv = 2.26 x 106 J/kg; cwater = 4186 J/(kg Co) a. 6060 J/K b. 6070 J/K c. 6320 J/K d. 6330 J/K 2. Relevant equations ΔS=ΔQ/T Q=mcΔT Q=mL 3. The attempt at a solution heat is needed to get the water to the boiling point 100C or 373K and then heat is needed to vaporize the water ΔS=(mcΔT+mL)/T ΔS=(1kg*4186J/kg*23K+1kg*2.26x10^6)/373 ΔS=6320 and the answer key says it is supposed to be 6070 what am I doing wrong?