a) One mole of ice is warmed from 220 K to 300 K at constant pressure of 1 bar.

Question

a) One mole of ice is warmed from 220 K to 300 K at constant pressure of 1 bar. Find the enthalpy change (delta H) for this process. b) If we assume that the volume of the ice/water does not change significantly during the process in part a, what is the energy change (delta U)? c) In fact, when the ice melts the density changes from 0.9167 g/cm^3 to 1.000 g/cm^3. If we assume that the volume change is due entirely to the density change (that is, neglect thermal expansion of the ice/water), what is the difference between the enthalpy change and the energy change during the process? Is this a significant difference, compared to the total energy change?

Explanation / Answer

a)delta H = C dT = 1 cal/(K·g) x 18 x (300-220) x 4.184 = 6024.96 J b)delta U =6024.96 J c) V=m/rho difference = 18((1/0.9167 - 1)x 10^-3)L x 0.9869 atm = 0.001614 J

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