suppose 1.00 mol of ice at -30.0c is heated at ... QuestionSuppose 1.00 mol of ice at -30.0C is heated at atmospheric pressureuntil it is converted to steam at 140.C. Calculated Q, W, ΔH, andΔU for this process. For ice, water, and steam, Cpm = 38.0, 75.0,and 36.0 J/mol K, respectively, and can be taken to beapproximately independent of temperature. ΔHfus for ice is 6.007 kJmol , and ΔHvap for water is 40.66 kJ mol . Use the ideal gas lawfor steam, and assume that the volume of ice or water is negligiblerelative to that of 1 mol of steam.
