Suppose we initially have a high-temperature substance, such as a hot piece of metal Mand a low-temperature substance, such as cool water W.
And as we'll learn in another episode, the extremely high specific heat capacity of water is due to the breaking in formation of hydrogen bonds that are associated with relatively small changes in temperature.
Calorimetry is performed with a calorimeter. In more recent calorimeter designs, the whole bomb, pressurized with excess pure oxygen typically at 30atm and containing a weighed mass of a sample typically 1—1. The energy produced by the reaction is trapped in the steel bomb and the surrounding water.
Well, the greatest factor is probably that we use the specific heat capacity of pure water instead of the saltwater that we actually created. The specific heat of water is approximately 4.
And how do we know the specific heat capacity? Determine the specific heat and the identity of the metal. To me, the coolest part of this is where the heat actually comes from. And what's even more awesome, if you ask me, is that we can actually figure out exactly how much heat will be released by this reaction.
Since the solution is aqueous, we can proceed as if it were water in terms of its specific heat and mass values. Then there's sodium hydroxide, another substance that I wouldn't wish to be on my worst foe, although, I'm glad we have it.