Heat Capacity and Temperature Change

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Homework Help Overview

The problem involves two metals with identical masses and initial temperatures being placed into water at a lower temperature. The focus is on understanding how the different heat capacities of the metals affect the temperature change of the water.

Discussion Character

  • Conceptual clarification, Assumption checking

Approaches and Questions Raised

  • Participants discuss the relationship between heat capacity and energy transfer, with one suggesting that the metal with the higher heat capacity will release more energy into the water. Others question the assumption that temperature changes (Δt) will be identical for both metals.

Discussion Status

There is an ongoing exploration of the implications of heat capacity on temperature change, with participants examining the conditions under which the temperatures are measured and the potential for different final temperatures for the metals and water.

Contextual Notes

The problem lacks specificity regarding the timing of temperature measurements after the metals are introduced to the water, which raises questions about thermal equilibrium and the conditions of the experiment.

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Homework Statement



Two metals of identical masses and initial temperatures are dropped into water which has a lower temperature than the metals. Both the water and the metals have the same mass.

One metal has a higher heat capacity than the other metal.

Which metal will change the water temperature the most?

Homework Equations



q=mcΔt

The Attempt at a Solution



Because it appears that all variables to the right of "q" are equal except c, it appears that the metal with the higher heat capacity will result in a higher "q" - it will release more energy into the water (since the water is cooler and heat flows from objects of higher to lower heat).

Therefore, it appears that the metal with the higher heat capacity will affect the temperature of the water more.
 
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Therefore, it appears that the metal with the higher heat capacity will affect the temperature of the water more.
That sounds right.

Because it appears that all variables to the right of "q" are equal except c, it appears that the metal with the higher heat capacity will result in a higher "q" - it will release more energy into the water (since the water is cooler and heat flows from objects of higher to lower heat).
That does not sound quite right. Δt will likely not be identical for the different samples.

(This could be made into a trick question, but as it stands I think it is meant to be straightforward.)
 
NascentOxygen said:
That does not sound quite right. Δt will likely not be identical for the different samples.
? Why not? How could they end up with different temperatures?

AM
 
Andrew Mason said:
? Why not? How could they end up with different temperatures?

AM

The problem is not specific about when the temperatures are measured after dropping the samples into the water. Is it one second after? One minute? When everything has reached thermal equilibrium?
 
Andrew Mason said:
? Why not? How could they end up with different temperatures?
The water warms while the metal cools. I assume separate cooling vessels.
 

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