Another URGENT HELP problem: Steam to Ice 1. The problem statement, all variables and given/known data How many J of energy must be removed when 127.0 g of steam, at a temperature of 153.0°C, is cooled and frozen into 127.0 g of ice at 0°C? Take the specific heat of steam to be 2.1 kJ/(kg·K). 2. Relevant equations Q1 = mc(delta T) <---- c= heat capacity of steam Q2 = mLv Q3 = mc(deltaT)<---- c=heat capacity of water Q4 = mLf 3. The attempt at a solution first I converted grams to kilograms and got .127kg for the mass then I follwed through with my equations Q1 = (.127)(2100)(153-100)= 1.4135E4 Q2 = (.127)(2259.36)= 2.869E2 Q3 = (.127)(4186)(100-0)= 5.316E4 Q4 = 4.241E4 I added these up and got a total Q of 1.10E5, what am I doing wrong?