Does same amount of heat absorbed cause the same changes of temperature in the same amount of different liquids? Explain.

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To answer your question we will assume certain things here.

  1. Assume $C_p = C_v$ for most liquids, where $C_p$ is the heat capacity at constant pressure, and $C_v$ is the heat capacity at constant volume.
  2. Assume that $C$ is constant with respect to temperature, which is not the case in most real fluids. Here, in order to leave out the integration, we assume that it is a constant.


$Q = C\Delta{}T$

As different liquids have different heat capacities, the same amount of heat supplied to the liquid would result in a different $\Delta{}T$, the temperature change.

The higher the heat capacity, the more heat is required to raise a unit mass(or mole) of substance by a unit temperature. Likewise, more heat has to be removed from the unit mass of substance in order to decrease the temperature by a unit temperature.

In other words, the higher the heat capacity, the more "reluctant" it is to change its temperature, for the same amount of heat supplied.

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    $\begingroup$ As examples, water has a heat capacity of 75 J/mol (to raise by 1 degree), while methanol is $\endgroup$ – Jon Custer Oct 2 '14 at 16:31

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