Calculation of entropy change for melting ice

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SUMMARY

The entropy change for melting 1 mole of ice at 268 K to form water at 323 K can be calculated using the enthalpy of fusion and the heat capacities of ice and water. The entropy change during the phase transition is determined by the formula delta(S) = delta(Q)/T, where delta(Q) is the heat absorbed. To account for the temperature change, one must integrate the heat capacities over the temperature range, applying the formula for variable temperature conditions.

PREREQUISITES
  • Understanding of thermodynamic concepts such as entropy and enthalpy
  • Familiarity with the heat capacities of substances
  • Knowledge of integration techniques in calculus
  • Basic principles of phase transitions in thermodynamics
NEXT STEPS
  • Learn how to calculate entropy changes using variable temperature conditions
  • Study the integration of heat capacities over temperature ranges
  • Explore the concept of enthalpy of fusion and its applications
  • Review thermodynamic equations related to phase changes and temperature effects
USEFUL FOR

Students in thermodynamics, chemistry, and physics, particularly those preparing for exams involving calculations of entropy and phase transitions.

chriswilson
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Homework Statement


Calculate the entropy change when 1 mole of ice at 268 K is melted to form water at 323 K. The heat capacity of ice is 3.8 J K-1 kg-1 and that of water is 75 J K-1 kg-1. The enthalpy of fusion of ice at 273 K is 6.02 kJ mol-1.

I know the entropy change by the melting of the ice is given by

delta(S)=delta(Q)/T

and that this is worked out by the enthalpy of fusion.

My question is how do I calculate the entropy change caused by the change in temperature since it is not at a constant temperature does this mean the first equation cannot be used?

Also this isn't a homework question it is an exam question from a previous year and my exam is tomorrow.
 
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Relate delta(Q) to temperature and integrate.
 

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