We are making silver!!!

Today we started off class by going over question #3 on the SuperMole Fun worksheet. The point of this problem is to find the amount of bacteria tissue (C5H7O2N) produced. In the problem you are given the kg of waste to start (10000 kg). You need to convert this into NH4+ ions so you multiply by 3.o kg NH4+ / 100 kg waste. Since the problem says the waste water contains 3% NH4+ ions, we can assume 100 kg. After converting to NH4+, multiply by 1000g / 1 kg so the equation is converted to grams. Next, you find the molar mass of NH4+, which is 18.04. Multiply the equation by 1 mol NH4+ / 18.04 g NH4+ to convert it into moles. After this you use the conversion factor 1 mol C5H7O2N / 55 mol NH4+ to convert the equation into moles of C5H7O2N. Next, you find the molar mass of the bacterial tissue which is 113 g and use the conversion factor of 113 g / 1 mol C5H7O2N to convert the equation into grams. The grams of bacterial tissue produced should be 34000 g. Once you have found this, multiply it by 0.95 (95%) because in the problem it says that only 95% of ammonium (NH4+) ions are consumed by the bacteria. If you had some trouble following this, the answers and work are posted here. After going over the worksheet, we started our Copper and Silver Nitrate Lab by going over the pre lab and procedures. This lab is going to take multiple days, so we haven't finished it yet, but it is due on tuesday of next week. Also, our class could probably make a huge profit by saving all our silver from the lab, just throwing that out there.

Everyone better watch the Bears own the Dolphins tonight. And the next scribe is...

Faith S.

A New Hope for Stoichiometry (Chemistry Honors Vs. Chemphys)

Today we continued our Intro to Stoichiometric Calculations. We had a very heated discussion about how Mr. Lieberman did not post the answers to the Intro To Stoich 1 worksheet until it was past some of our bedtimes (claims were made of that time being before 6:45 pm.... :s). Anyway after we got over that hump, we dove into a practice/example problem that Mr. Lieberman did on the board. It went a little like this:
Reaction #1: CaC2 + 2H2O --> Ca(OH)2 + C2H2
Then we plugged C2H2 into a combustion reaction: (It is balanced..DUH) 2C2H2 + 5O2 --> 4CO2 + 2H2O
Mr. Lieberman then posed to the question of: If .60 grams of CaC2 reacts, how many grams of H2O will form? ( Use the balanced combustion equation above)


The converstions look like this:

In the end you end up with .17 moles of H2O. Soon after this we witnessed the astonishing demo of Evil KinMOLble! This unlucky or lucky, (I'm not sure what was going through his head..... probably AAAAAAAAAAAAAAAHHHHHHHHHHHHH!!!!!!!!!!!!!) It was the projectilation of Mr. Mole from Mr. Lieberman's Mole Cannon using the combustion. The combustion was caused by the ignition of Acetylene from the reaction of H2O and CaC2(I think not sure on this). After that first demo, we took our short little quiz on Stoichiometry. Lastly, as a conclusion to our class period, Mr. Lieberman armed the launcher once again and fired it into the ChemPhys classroom next door. Causing complete academic Armageddon in the science wing. (ok I exhaggerated a little). Check out the Video in the post underneith this.

The next scribe is Tom btw.

Stoichiometry

We started class today with an in-class blowup. With the help of the whole class believing and some intense movie-quality diving out of the way, we got the magical blowing up elves to make the magical paint can blowup.
Then we got down to business. We went over the notes of the first two slides in Stoich.

Stoichiometric calculations

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To figure out the problem on the second slide, you need to know that the mole ratio = the moles wanted/the moles given. We also had a worksheet given to us along with the objectives and calendar. The next scribe is going to be Erica G.