Calculating Final Temp of a mixture

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SUMMARY

The discussion revolves around calculating the final temperature of a mixture consisting of 22.0 g of ice at -12.0°C and 120.0 g of water at 86.0°C, assuming no heat loss to the surroundings. The relevant heat capacities are 2.08 J/g°C for solid water (ice) and 4.18 J/g°C for liquid water, with an enthalpy of fusion of 6.02 kJ/mol for ice. Participants emphasized the need to apply the principles of heat transfer and phase changes to arrive at the final temperature of the mixture.

PREREQUISITES
  • Understanding of heat transfer principles
  • Knowledge of specific heat capacities
  • Familiarity with phase changes and enthalpy of fusion
  • Ability to perform calculations involving mass, temperature change, and energy transfer
NEXT STEPS
  • Learn how to apply the heat transfer equation Q = mcΔT
  • Study the concept of phase changes in thermodynamics
  • Explore the calculation of final temperatures in mixtures
  • Review the enthalpy of fusion and its application in thermal calculations
USEFUL FOR

This discussion is beneficial for students studying thermodynamics, particularly those tackling heat transfer problems in chemistry and physics courses.

viper2308
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Homework Statement


A 22.0 g sample of ice at -12.0°C is mixed with 120.0 g of water at 86.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol


Homework Equations


I am not at home and don't have my book and the homework is due at 6:30 tonight so I can't figure out how to do this.


The Attempt at a Solution


I have no idea what equations to use to even try an attempt. Please Help.
 
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