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Question:

If equal masses of water and aluminum interact thermally, will the final temperature be closer to the...?

... initial temperature of the water or the initial temperature of the aluminum? Why?

Answer:

Let's say the aluminum starts out at a higher temperature than the water. The aluminum cools down by 1°C, which means it loses energy (Q = mcΔT, where ΔT = 1°C). That energy goes to the water, warming it up. Since Q is the same for both water and aluminum, and m is the same for both, all that matters is the heat capacity c. Water has a higher heat capacity than aluminum, so for the same Q it must have a smaller ΔT. This process continues until both have reached the same T. From the above paragraph, you should be able to figure out if the final T is closer to the initial water temp or the original aluminum temp.
The correct equation is: dQ = m*c*dT As dQ (substitute of thermal potential) and mass are the comparable, the equation may well be rewritten as: c*dT=consistent So a cloth with a decrease specific warmth skill could have a much better improve in temperature. The question has already suggested this yet now all of us be attentive to they are inversely proportional. to that end: c of aluminium/c of copper = dT of aluminium / dT of copper 0.22/0.092 = proportionality consistent = 2.39 So copper would be 2.4 circumstances warmer than aluminium (or aluminium would be 0.40 two circumstances warmer than copper).

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