Problem 3. (30 pts) A thermally isolated 1.000 mole of ice is superheated to +10

Question

Problem 3. (30 pts) A thermally isolated 1.000 mole of ice is superheated to +10 ºC (283 ºK) at 1 atm. The system is allowed to come to equilibrium. Useful thermodynamic properties of water are: Heat of melting = 6,007 J/mol, Heat of boiling = 40,660 J, molar specific heat of ice = 38.07 J K-1 mol-1 , molar specific heat of liquid water = 75.4 J K-1 mol-1, molar specific heat of steam = 33.76 J K-1 mol-1. (You will need to choose which of these properties are useful and which can be ignored.)

a. (5 pts) What will the equilibrium conditions be in terms of pressure and temperature?

b. (10 pts) How many moles of ice will turn to liquid water when the water comes to equilibrium?

c. (15 pts) What is the change in entropy of the system? Be sure to indicate whether the overall change in entropy is positive or negative.

Explanation / Answer

Ans:

a.) Equilibrium conditions are 1 atm and 283 K.

c.) Entropy of the system is negative, since the entropy of ice is more than water.

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