The first topic was the first law of thermodynamics, or the law of

conservation of energy. This law states that in a reaction, energy cannot be

created or destroyed by any ordinary physical means. We emphasized this law

through means of the system and surrounding in a reaction. We also noticed

that a system and a surrounding are sometimes interchangeable. For example,

we observed that a hungry student could be either a system or a surrounding.

It is important to notice that according to the law of conservation of

energy, the energy lost system, has to equal the energy gained in the

surrounding (or vice versa). Therefore: delta E system ñ delta E surrounding

= 0

The second topic we covered was how to calculate the amount of heat

(q) lost in a system/gained in the surrounding (or vice versa) by using

specific heat (S): the amount of energy it takes to heat 1 gram of a

substance 1 degree Celsius (measured in Joules/grams-Celsius). In order to

calculate q we derived an important equation: q= (the change in Temperature)

(specific heat of substance)(mass of substance), or (delta T)(S)(M H2O) Also,

it is important to remember that because S is an intensive property; the

amount of the substance does not matter.

Finally, the third topic we learned was heat capacity (C), or q

needed to raise the temp a given amount of a substance 1 degree Celsius.

(measured in Joules/degree) The C of a substance is the result of (the

specific heat)(mass of the substance), or (S)(mass). Heat capacity is an

extensive property, which means that the amount of matter of substance does

matter (no pun intended!!) :)

Hint: C= S(Mass) Therefore, if given the Heat Capacity of a substance and

delta T, it is a shortcut to calculate q.