Consider the reversible melting of 1 mol of ice in a large, isothermal water bat

Question

Consider the reversible melting of 1 mol of ice in a large, isothermal water bath at 0oC and 1 atm pressure. The enthalpy of fusion of ice is 6.01 kJ/mol. Calculate the entropy change in the surrounding (Ssurr).

Consider the eversible melting of 1 mol of ice in a large isothermal water bath at 00C and 1 a pressure. The enthalpy of fusion of ice is 601 m Calculate the entr p change he unding u (Refer to the last part "PhaseTransitions" of 175GibbsFreeEnergy in the textbook) 22.0 J/molk -22.0 J/molK O 0.00022 J/molK 0-0.00022 J/moIK

Explanation / Answer

Suniverse = Ssurr +Ssys

at constant temperature or isothemal ,

Suniverse = 0 = Ssurr +Ssys

Thus

Ssurr = -Ssys

H fusion = 6.01 KJ/ mol = 6010 J/mol

T = 0oC = 273K

Ssys = Hfusion/T = 6010/273 = 22.0 J/molK

Ssurr = -Ssys = -22.0 J/molK

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---