# chemistry

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how much heat (in KJ) is evolved in coverting 1.00 mol of steam at 135.0 degrees celcius to ice at -45.0 degrees celcius? the heat capacity of steam is 12.0 J/g * C and ice is 2.09 J/c * C.

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35*

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You do this in steps. First, note the correct spelling of celsius.
q1 = heat to move steam from 135 C to 100 C.
q1 = mass x heat capacity steam x (Tfinal-Tinitial)=?? where, in this case, Tfinal = 100 and Tinitial = 135.

q2 = heat evolved in condensing vapor at 100 to a liquid.
q2 = mass x heat of vaporization=??

q3 = heat evolved in cooling water from 100 C to 0 C.
q3 = mass x heat capacity of water x (Tf-Ti) = ??

q4 = heat evolved in freezing the ice (from liquid to solid) but leaving the T at 0 C.
q4 = mass x heat of fusion = ??

q5 = heat evolved in moving T of ice from 0 C to -45 C.
q5 = mass x heat capacity ice x (Tfinal-Tinitial) = ??

Now add q1+q2+q3+q4+q5, and change the total from Joules to kJ. Post your work if you get stuck.