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Suppose you have 1 kg each of iron, glass, and water, and all three samples are at 10°C.
(a) Rank the samples from lowest to highest temperature after 100 J of energy is added to each by heat.
(b) Rank them from least to greatest amount of energy transferred by heat if enough energy is transferred so that each increases in temperature by 20°C.

Respuesta :

cjmejiab

To solve this problem it is necessary to apply the concepts related to heat exchange and Entropy.

The temperature and mass remain constant, therefore the entropy values will be the only ones to change.

Of the three elements given their entropy values are given by

[tex]\Delta S_{iron}=0.45J/gmC[/tex]

[tex]\Delta S_{glass}=0.8J/gmC[/tex]

[tex]\Delta S_{water}= 4.186J/gmC[/tex]

Part A) From thermodynamic theory we know that temperature is inversely proportional to entropy

[tex]T = \frac{E}{\Delta S} \rightarrow[/tex] Energy remains constant

[tex]\Delta t \propto \frac{1}{S}[/tex]

Therefore the order would be

Lowest Temperature= Water

Medium Temperature= Glass

Highest Temperature=Iron

Part B) In the case of Energy the opposite happens because it is proportional to the entropy, then

[tex]E = T(\Delta S) \rightarrow[/tex]Temperature is constant

[tex]E \propto S[/tex]

Lowest Energy = Iron

Medium Energy = Glass

Highest Energy = Water

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