How much heat ( in kilojoules) is released for converting...?

Question

100.0 liters of water steam collected at 127.0 degrees celsius ( under 1 atm) to ice at -20.0 degrees celsius. (Molar mass: O = 16.00 g, H = 1.008 g. The specific heat of ice is 2.03 J/g-degrees celsius, the specific heat of water is 4.184 J/ g- degrees celsius, the specific heat of steam is 1.99 J/g-degrees celisius. the heat of fusion is 6.01 kilojoules for water, and he heat of vaporization is 40.79 kilojoules for water)

Answer 1

You're missing the density of steam. Suppode the density is d g/mL. 127C - 100C = 27degC. First cool the steam to 100C:

100Lsteam x 1000mLsteam/1Lsteam x d gsteam/1mLsteam x 27degC x 1.99kJ/g-degC = The amount of heat liberated

And you would need the g steam, water, and ice to go on with the rest of the problem.