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Tema [17]
3 years ago
7

A 57.07 g sample of a substance is initially at 24.3°C. After absorbing of 2911 J of heat, the temperature of the substance is 1

16.9 CWhat is the specific heat (SH) of the substance?
Chemistry
1 answer:
icang [17]3 years ago
8 0

Answer:

Approximately 0.551\; \rm J\cdot kg^{-1} \cdot \left(^\circ\! C \right)^{-1}.

Explanation:

The specific heat of a material is the amount of energy required to increase unit mass (one gram) of this material by unit temperature (one degree Celsius.)

Calculate the increase in the temperature of this sample:

\Delta T = (116.9 - 24.3)\; \rm ^\circ\! C= 92.6\; \rm ^\circ\! C.

The energy that this sample absorbed should be proportional the increase in its temperature (assuming that no phase change is involved.)

It took 2911\; \rm J of energy to raise the temperature of this sample by \Delta T = 92.6\; \rm ^\circ\! C. Therefore, raising the temperature of this sample by 1\; \rm ^\circ\! C (unit temperature) would take only \displaystyle \frac{1}{92.6} as much energy. That corresponds to approximately 31.436\; \rm J of energy.

On the other hand, the energy required to raise the temperature of this material by 1\; \rm ^\circ\! C is proportional to the mass of the sample (also assuming no phase change.)

It took approximately 31.436\; \rm J of energy to raise the temperature of 57.07\; \rm g of this material by 1\; \rm ^\circ C. Therefore, it would take only \displaystyle \frac{1}{57.07} as much energy to raise the temperature of 1\; \rm g (unit mass) of this material by 1\; \rm ^\circ \! C\!. That corresponds to approximately 0.551\; \rm J of energy.

In other words, it takes approximately 0.551\; \rm J to raise 1\; \rm g (unit mass) of this material by 1\; \rm ^\circ \! C. Therefore, by definition, the specific heat of this material would be approximately 0.551\; \rm J\cdot kg^{-1} \cdot \left(^\circ\! C \right)^{-1}.

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