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A sample of ice weighing 16.09 g, initially at -38.5°C, is heated to 140.0°C at a constant pressure of 1.00 atm. Calculate q, w, E, H, and S for this process. The molar heat capacities (Cp) for solid, liquid, and gaseous water (37.5 J K-1 mol-1, 75.3 J K-1 mol-1, and 36.4 J K-1 mol-1) respectively-are assumed to be temperature independent. The enthalpies of fusion and vaporization are 6.01 kJ/mol and 40.7 kJ/mol, respectively. Assume ideal gas behavior.

2007-04-17 21:47:35 · 2 answers · asked by FaceFullofFashion 6 in Science & Mathematics ➔ Chemistry

2 answers

have no idea

2007-04-18 02:02:34 · answer #1 · answered by Anonymous · 1⤊ 1⤋

q = sum of ms delta t and fusion

= 16.09*(37.5*38.5 +6.01+ 75.3*100 +40.7+ 36.4*40) /18

= 9 364.79119 kJ

2007-04-18 05:09:41 · answer #2 · answered by ag_iitkgp 7 · 1⤊ 0⤋