Welcome to 2020 and welcome to the next cool topic (or hot, it’s just the reverse of cool).

Thermochemistry involves heat (thermal-underwear keep the heat inside, the old outside).  We will figure out how much energy it takes to melt ice cubes of different sizes.  We will also see that melting other substances, like gold, or iron, take different amounts of energy than each other, or than water.

We will also learn to measure how much energy it takes to warm things up.  We can warm solids, or warm up liquids, or even warm up gases.  All substances (in all phases) take different amounts of energy to warm up by a certain number of Kelvin units of temperature.

We will further learn that cooling things down requires the removal of the same amount of energy it takes to warm them up by that same number of Kelvins.

We will learn about energy units called Calories (which you eat), scientific calories (which are 1000x smaller), joules – which are way cool, and kilo-joules (which are 1000x bigger than joules).  We’ll convert them back and forth easily with one-step unit conversion math.

Finally, we will see that every substance has a “specific heat capacity constant”, or the amount of energy it takes to warm up one gram of that pure stuff by one Kelvin.  It’s got the weirdest units of the whole year too.

And we will use three funky formulas, shown below.  It’s all good, and so are both of the labs (although the Doritos Lab does smell a bit gross).  Get ready to learn A LOT.  Chem starts anew, vacation is over.

q = mCΔT          .           q = mHF                 .       q = mHV

You will be expected to read the BASICS and bring a calculator each day, or you will fall further behind than ever before.  We will start to go a bit faster than we have been, we’ll do more math, more thinking, and become better people each day.

Smile, today is the first day of the rest of your life.

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