Hydrates Lab

First, approximately 5g of CuSo4 5H2O was placed into a test tube. (Since it was in chunks, ours started out as 1.5625g)

Next, the tube was held over a Bunson Burner until a chemical reaction took place in the contents of the tube. The color of the CuSo4 5H2O changed from blue to white! Gas escaped the contents.

The mixture was measured. From this, it was noticed that was lighter than before! (That was the weight of the gas contained in the CuSo4 5H2O)
The chemical now weighed 1.02g.

This gives the conclusion that the amount of weight lost from the mixture was .56g.

Just to experiment some more, we further squirted some water into the tube with the mixture. To our surprise, it changed colors back to blue! Neat!

Popcorn lab!

For this lab, we made-yes-POPCORN!

Here, popcorn kernels (approximately 25-30) were placed in a 100 ml beaker with enough vegetable oil in it to cover the bottom (the oil came out fast, so we had a little bit more!). This was covered by an aluminum foil film. 

From here the Bunson burner was turned on just below the beaker, boiling the vegetable oil. It was noticed that the kernels appeared to be releasing air through their tips! 

Soon, the popcorn started to pop and eventually, vapor was collecting in the upper part of the beaker, just under the aluminum and releasing through holes poked into it. The popcorn appeared to be very white!

After turning off the burner, the beaker was left to cool off for several minutes. Finally, the beaker was weighed. At the end of the project, the solution weighed less than the beginning.

Mole Activities/Lab

THE MOLE

No, not on your face! The mole, in scientific measurement, is a number! It is shown as:

 6.02 × 10²³

Each element measures a different amount, when it comes to the mole. Ever wonder why there are two numbers on each element when they're in their place on the periodic table? The first number is, of course, the number of the element, but what's that other number for? That's how much of that element (in grams, or abbreviated as "g") measures into 1 mole (abbreviated as "mol"). So for example, 1 mole of Aluminum would be 26.982g.

So how do I calculate figure out how many moles are in a certain amount g?
For example, you are trying to find how many moles are in 15 grams of lithium. Here, you will multiply by 15 at the beginning of the equation. Next, there wil be a fraction of 1 mole over 6.94gLi. Divide the fraction and multiply the answer by 15. This should bring you to the answer of 2.16 moles.

(1 mol)

           15 g × (6.94 g Li) = 2.16 mol

So what if I wanted to calculate how many g are in a certain amount of moles?
This equation will look very similar, but each part of this equation will have a different location. Observe.
Example: How many grams are in 2.4 moles of Sulfur?

(32.06gS)

2.4 mol × (1 mol) = 76.94 g S

Some fun facts about the mole!

• One mole of paper would make a stack that would reach to the moon more than 80 billion times
• A one liter bottle of water contains 55.5 moles of water
• One mole of seconds is about 19 quadrillion years, 4,240,666 times the age of the earth, or 954,150 times the age of the universe itself