Given that the specific heat capacities of ice and steam are 2.06 J/g degrees C and 2.03 J/g degrees C, respectively, calculate the total quantity of heat evolved when 10.0 g of steam at 200 degrees C is condensed, cooled, and frozen to ice at -50 degrees C.
Chemistry - DrBob222, Wednesday, April 27, 2011 at 5:18pm
q1 = heat released on cooling steam from 200 C to 100 C.
q1 = mass steam x specific heat steam x (Tfinal-Tintial). Tfinal = 100, Tinitial = 200
q2 = heat released when steam is condensed at 100 C to liquid water at 100 C.
q2 = mass steam x heat vaporization
q3 = heat released in cooling liquid H2O from 100 C to zero C.
q3 = mass H2O x specific heat H2O x (Tfinal-Tinitial)
q4 = heat released on freezing water at zero C to ice at zero C.
q4 = mass water x heat fusion
q5 = heat released in cooling ice at zero C to ice at -50C.
q5 = mass ice x specific heat x (Tfinal-Tinitial)
Total Q = q1 + q2 + q3 + q4 + q5