1) One mole of ice is warmed from 220 K to 300 k at constant pressure of 1 bar.
ID: 594192 • Letter: 1
Question
1) One mole of ice is warmed from 220 K to 300 k at constant pressure of 1 bar. Find the enthalpy change for this process 2) If we assume that the volume of the ice/water does not change significantly during the process in #1 what is the energy change? 3) When the ice melts the density change from .9167 g/cm^3 to 1.000 g/cm^3. If we assume that the volume change is due entirely to this density change (that is we neglect thermal expansion of the ice/water), what is the difference between the enthalpy change and the energy change during theis process? Is this a significant difference, compared to the total energy?Explanation / Answer
pressure is constant so V/T=constant
V1=RT/P =0.0183 m3
V2=V1T2/T1 =0.025 m3
H=P(V2-V1)=670 J
b)energy change=H =670 J
c)difference between the enthalpy change and the energy change during theis process
=P*18*10-3(1/916.7 -1/1000)=10^5*18*10^-3*9.08*10^-5 =0.164 J which is very low
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