This week, We learned about the concepts of Dalton's theory.
On Monday, our class did a simulation on Dalton's theory in
the computer game. The first part of the game (Priestley) consisted of burning calx. As 7.39g of the
100g calx was burned, only 92.61g remained. We then had to use 200g of calx. With
conservation of mass it would be understandable that the mass would be two
times as much than the product from the first trial. The change in mass was
14.78g from the 200g calx. Therefore, depending on the mass of a substance
burning, it loses mass at a proportional rate. We also had to find the volume
of gas produced after burning the calx. I noticed that more mass was burned,
the more volume the calx would be surrounded in. Using the 100g, the volume of
gas came out to be 5.171L, and then using the 200g, the volume of gas came out
to be 10.34L. So since there is only half of the mass of calx left, the volume
doubled. Also, the volume of gas changed at a proportional rate to the rate at
which the mass of calx changed. With this simulation, we learn that all chemical
reactions occur in a fixed ratio. 
The next experiment was the Lavoisier portion. This is where
the phlogiston and the oxygen were tested at burned at different rates to see
how they would change in mass or volume. First, 1/3 of the phlogiston was
burned. To begin with, both started out with volumes of 6L and they were both
in separate beakers , which had tubes connecting to a center beaker, which is
where the gas would go. As the oxygen and phlogiston burned, 5L for both were
left. Next, as 2/3 of the phlogiston were burned, 4 L for both oxygen and
phlogiston were left. But then, when all the phlogiston was burned, only half
of the phlogiston was used up so that 3L of oxygen were left. This would mean
that the phlogiston burned quicker, two times to be exact. We were then later
told that they renamed phlogiston to hydrogen simply meaning “water maker”.
Lastly, we worked on the Diamond and Charcoal lab. We started
out with 0.20g of charcoal and diamond and kept the mass of oxygen at 1.06g and
volume at 0.74L constant (charcoal and diamond were tested individually). The
mass of the oxygen decreased from 1.06g to 0.73g as the subtracted amount went
to the 0.20g of charcoal, thus increasing the mass of charcoal to 0.53g. Next,
0.40g of charcoal was tested with the same volume of gas (0.74L). Then, the
mass of gas decreased from 1.06g to 0g and the volume dropped from 0.74L to 0L.
Therefore, with twice the mass, the rate at which volume dropped doubled, hence
the rate at which charcoal's mass increased. It was interesting to see that while
charcoal and diamond look so different, they do still share chemical
properties. I learned that they were related because of Jimmy Neutron! In
conclusion, when something is taken away it is always somewhere else due to it
being in a closed system and that chemical reactions occur at a fixed ratio.
We later on in the week focused on the things we learned in
class on Monday and we had an assessment on Friday. I am not sure how I did,
but I know I struggled in some areas that I missed that week.
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