Heat Capacity and Temperature Change

AI Thread Summary
In the discussion about heat capacity and temperature change, it is established that two metals with identical masses and initial temperatures are placed in cooler water. The metal with a higher heat capacity is expected to release more energy into the water, thus affecting its temperature more significantly. However, there is a debate regarding the measurement of temperature changes, as the time at which temperatures are assessed can influence the results. It is noted that the water will warm while the metal cools, leading to potential differences in final temperatures. The conversation highlights the importance of thermal equilibrium in understanding the heat transfer process.
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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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