Map Sapling Learning A 0.5530-kg ice cube at -12.40 oC is placed inside a chambe

Question

Map Sapling Learning A 0.5530-kg ice cube at -12.40 oC is placed inside a chamber of steam at 365.0°C. Later, you notice that the ice cube has completely melted into a puddle of water. If the chamber initially contained 6.910 moles of steam (water) molecules before the ice is added, calculate the final temperature of the puddle once it settled to equilibrium. (Assume the chamber walls are sufficiently flexible to allow the system to remain isobaric and consider thermal losses/gains from the chamber walls as negligible.) Number

Explanation / Answer

C of H20 (s): 37.7 J/(mol K)
C of H20 (l): 75.3 J/(mol K)
enthalpy of fusion of H20: 6.01 kJ/mol

27.8 J/(mol K) at 400 °C or 2.02J g¯1K¯1.

calculate how much energy must be absorbed to melt the ice cubes:

here mass of ice = 0.5530 kg = 553 g

553 g/18 g/ mol= 30.7 mole

{(30.7-mol x 12.40 °C x 37.7-J/mol*°C) + (30.7-mol x 6010-J/mol) + [30.7-mol x (Tf - 0 °C) x 75.3-J/mol*°C]} = -{6.910-mol (365 °C - Tf) x 27.8-J/mol*°C }

14351.636 + 184507 + 2311.71 Tf = - 70115.77 + 192.098Tf

268973.77 = 2119.612 Tf

Tf = 126.89 degree

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