Specific Heat Capacity is a topic that is studied at A2 level in the UK (16+)

The specific heat capacity of a solid or liquid is defined as the heat energy required to raise the temperature of unit mass of a substance by one degree.

At A level you have to use the following equations to perform calculations involving change of energy

Q = mc

where m is the mass of the substance, c is its specific heat capacity and is the change in temperature

Q = ml

where l is specific latent heat and m is the mass of substance changing state

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The internal energy (sometimes called the random thermal energy) of a substance is the sum of its kinetic energy and potential energy. Potential energy is due to the interaction of neighbouring particles, this is therefore very significant in solids and liquids but less so in gases. Kinetic energy is due to the movement of the particles in the substance.

You should be able to define the specific heat capacity of a substance as being the quantity of energy required to raise the temperature of 1kg of the substance by 1K.You should realize that the biggest changes in temperature of a given mass of a substance will occur in those that have low specific heat capacities - because it doesn't take much energy for them to get hotter!

You should be able to define specific latent heat as the energy required to change the state of 1 kg of the substance.You should be able to understand what is happening to the particles in a substance when heat is added to it or taken away

If the substance is remote from its melting or boiling point it will change temperature (getting hotter or colder) as the particles vibrate faster or slower on absorbing the heat energy - the kinetic energy component changes significantly the potential energy component is virtually the same.The amount of heat energy required to make a temperature change of 1K will depend on the mass of the substance (the more you have the more energy you will need, natch!) and what it is - some structures react to heat input more dramatically than others (this is indicated in the SHC 'c' of the substance) - low 'c' substances have particles that are easier to 'vibrate'!

If the substance is at its boiling/melting point the energy given/taken away will not be used to get hotter or colder. It will be used to change state. If absorbed (given to the substance) it will not make the particles vibrate any faster, but will make them freer from each other. If being taken away, again it will not change the vibration of the particles but rather will make them more structured - less free - and change their state to do that. So when latent heat is involved we are looking at the change of potential energy not kinetic energy.

When you do calculations involving heat being given and/or taken away remember to add up all of the components that have been 'given energy' and all of those that have 'given energy away' and equate them in an exchange of heat problem. No heat 'disappears' it gets transferred between the substances. Heat losses to the surroundings and equipment are usually ignored - but you may be asked why practical measurements differ from theoretical calculations.

Here is the link to the page that contains a PowerPoint on this topic