Finding the mass of iron using the heat equations

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To find the mass of iron that raises the temperature of 20.0 kg of water from 16°C to 18°C, the heat gained by the water equals the heat lost by the iron, expressed as q1 + q2 = 0. The specific heat of iron is 460 J/kg°C, while for water, it is 4190 J/kg°C. The calculations show that the mass of iron required is approximately 3.5 kg. The discussion also raises the question of the final temperature of the iron, emphasizing the need for equilibrium between the hot and cold substances. Understanding that they reach the same final temperature is crucial for solving the problem.
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Homework Statement


Calculate themass of iron at 100C that causes 20.0 kg of water to change temperature from 16C to 18C. C of iron is 460 J/kg C. The C for water is 4190. [/B]

Homework Equations


q1+q2=0
q=mct[/B]

The Attempt at a Solution


q1=-q2
mct=-mct
20(4190)(2)=-m(460)(100)
167600=46000m
3.5=m
 
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What's the final temperature of the iron? What was the temperature change of the iron?

Chet
 
That's my main issue right now because that is not given to me and I am having a hard time trying to figure how one would do that without the mass being given.
 
math989 said:
That's my main issue right now because that is not given to me and I am having a hard time trying to figure how one would do that without the mass being given.
If you put something hot in contact with something cold and let them equilibrate with one another, do they (a) reach different final temperatures or (b) reach the same final temperature?

Chet
 
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