How much heat is required to raise the temperature of 37.6 g of water from −45 C to 115 C?

Answer 1

q = (37.6 g)(2.09 J/gº)(45) = 3536 J to go from -45º to 0º

q = (37.6 g)(334 J/g) = 12,558 J to melt the ice

q = (37.6 g)(4.184 J/gº)(100º) = 15,732 J to raise temp from 0 to 100º

q = (37.6 g)(2260 J/g) = 84,976 J to turn liquid into steam at 100º

q = (37.6 g)(1.89 J/gº)(15º) = 1066 J to raise temp of steam 15º

Add up all the joules and get your answer. To convert to kJ, simply divide your answer by 1000