Solving Calorimetry Problem: Iron in Water

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SUMMARY

The calorimetry problem involves a 12g piece of iron at 80°C being dropped into 600g of water at 25°C. Using the equation q=mc∆T, where the specific heat of water is 4.184 J/g°C and that of iron is 0.44 J/g°C, the heat lost by the iron equals the heat gained by the water. By applying this principle, one can calculate the final equilibrium temperature of both substances.

PREREQUISITES
  • Understanding of the calorimetry equation q=mc∆T
  • Knowledge of specific heat capacities of substances
  • Basic algebra for solving equations
  • Familiarity with heat transfer concepts
NEXT STEPS
  • Calculate the final temperature using the heat transfer equation for both iron and water
  • Explore the concept of thermal equilibrium in calorimetry
  • Learn about specific heat capacities of other materials
  • Investigate real-world applications of calorimetry in various fields
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Students studying thermodynamics, chemistry enthusiasts, and educators teaching calorimetry principles.

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okay so i understand q=mc∆T and all but this problem really has me stumped

a 12g piece of iron (80°C) has been dropped into 600g of water (25°C)

the specific heat of water is 4.184J/g°C and iron's is .44J/g°C

what is the final temperature of the two?
 
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So you need to apply that equation for each substance. The heat lost by the iron will equal the heat gained by the water. They will both come to the same final temperature.

Try to set it up.
 

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