How can we identify that the absorption of heat has occurred?

For calorimetry problems, here’s the formula you need to use:

So Q is what you’re trying to find, the energy absorbed by the copper.

You already have the mass of the copper sample (60.0 g) and the change in temperature (80.0 - 20.0), which is 60.0 degrees Celsius). The only piece of information you’re missing is the specific heat capacity of copper. In my experience, this value is usually included in the question if the substance is not water. If not, you can look up the specific heat capacities of different substances online, or perhaps in a table at the back of your textbook:

Once you have that, you can solve for Q (make sure you always pay attention to your units!)

That is a thermodynamic problem.

You need to apply the first law of thermodynamics, which is (when applied to the copper block) :

ΔU=δQ−δW−ΔEc

As you consider the whole heating process to happen without any variation of the mecanichal energy and of the pressure, then ΔEc=0 .

Furthermore, the transformation is isobaric (pressure is constant), so δW=0 : you can then say that ΔU=ΔH.

So now you have ΔH=Q

You know the formula for ΔH in case of an isobaric transformation :

ΔH=cp∗mcopper∗ΔT and so you have at the end : Q=cp∗mcopper∗ΔT

with cp the isobaric capacity of copper : cp=385J.kg−1.K−1

Fill the equation with your data, and that’s your answer. All those thermodynamic problems are solved the same way : first law + enthalpy. Once you know the scheme, it’s over !

rise in temperature and the effect it has on our global weather patterns

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