Thermal Equilibrium: Solving for the Specific Heat of an Unknown Metal

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SUMMARY

The discussion focuses on calculating the specific heat of an unknown metal using thermal equilibrium principles. A 0.75 kg piece of metal at 200 degrees Celsius is placed on a 5 kg block of ice, resulting in the melting of 0.27 kg of ice. The specific heat of the unknown metal is determined to be 2114 J/kg, based on the formulas Q=mc∆T and Q=mL, where the specific heats of ice and water are 2000 J/kg and 4186 J/kg, respectively. The calculations involve understanding energy transfer and the latent heat of ice, which is 33.5 x 10^4 J/kg.

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Suppose a large block of ice (m=5kg) has a .75kg piece of hot(200 degrees C) metal placed on it so that in time, .27kg of ice melts, what is the specific heat of the unknown metal?

specific heat of ice - 2000 j/kg
specific heat of water - 4186 j/kg
Latent heat of ice - 33.5 x 10^4



Q=mc∆T, Q=mL
Q - Energy lost or gained.
m - Mass
c - specific heat
∆T - change in temp.
L - Latent Heat


Attempt:
Specific heat of 2114 j/kg
 
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I agree with your formulas, but not your answer. Can you show specifically what you did to come up with your answer?
 
ApexStudent1 said:
Suppose a large block of ice (m=5kg) has a .75kg piece of hot(200 degrees C) metal placed on it so that in time, .27kg of ice melts, what is the specific heat of the unknown metal?

specific heat of ice - 2000 j/kg
specific heat of water - 4186 j/kg
Latent heat of ice - 33.5 x 10^4
Why would you need to know the specific heat of water? What are your units for specific heat?

Answer these questions: How much heat is given to the ice (in Joules)? What is the final temperature of the metal? How many Joules per Kg of metal per degree change in temperature for the metal?

AM
 

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