Solving Calorimetry Problem: Iron in Water

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To solve the calorimetry problem involving a 12g piece of iron at 80°C dropped into 600g of water at 25°C, the principle of heat transfer is applied, where the heat lost by the iron equals the heat gained by the water. The specific heat capacities are crucial: water has a specific heat of 4.184 J/g°C, while iron's is 0.44 J/g°C. By using the equation q=mc∆T for both substances, the final temperature can be calculated. Setting up the equation involves equating the heat lost by the iron to the heat gained by the water. This approach will yield the final equilibrium temperature of the system.
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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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