Copper (II) Chloride and Iron Lab day 2

WOW!!!! Over night the reaction went wild!! There was this creepy weird orange stuff that looked like coral or something that you would find in the ocean on a reef! It grew on the nail!!! It looked pretty disgusting in all honesty! All of that stuff that grew on the nail was the copper! We had to take forceps to grip the nail and take water to get that product off the nail. Now the tedious part came! We had to siphon (suck up all the liquid) the solution the copper was in making sure to not suck up any product off. Then we had to add 25mL of HCl and siphon that off too. Then we had to add 25mL of water and siphon that off as well. The part that I probably scared me the most was worrying about if I sucked up any product! I wanted to make sure our results were as pure as they could get! So siphoning off three times made me feel like I was some surgeon operating on a heart! Now we just have to wait and let it dry!

Here are some pictures of the lab on day 2 below!

Copper (II) Chloride and Iron Lab day 1

This lab is overall pretty amazing! We first had to take the mass of the baby food jar and add copper (II) chloride in it. The powder was a pretty blue with sparkles. Then we added water in the jar, and we had to stir it with a stirring rod. Then we added the polished iron nail into the solution. Immediately we saw a reaction! The nail looked like it was being heated up because it looked like a yellow/orange kinda color that metal looks like when you're melting it. Then we just had to let it sit and wait for the reaction to finalize over night!

Here are some pictures below of the lab on day 1!

Weekly Quiz #1 for Stoichiometry

I made sure to do lots of practice questions in the multiple packets I printed off for this unit. In summary for Stoichiometry you basically find the limiting reagent and excess reagent. To do that you must take 2 elements/compounds with their given mass in grams. You must convert it both to moles in separate equations and then multiply that by the number of moles (coefficients!!!) for the element/compound you are trying to find and the number of moles of the element you are working on on the bottom of the fraction. Then you multiply that by the molar mass of the element/compound you are trying to find and put that over 1 mole. Once that is done, you look at which element/compound that produced the least amount of whatever element/compound that you're trying to find. The least one is your limiting reagent because that element/compound will run out first and limit the amount you can make in the other element/compound that you found. That will be your answer! :)

In the excess one (the element that produced the most amount of the element/compound), you basically do the same thing. However you take the limiting reagent amount (smallest number you found above) and convert that to moles. Then you multiply it by the molar fraction with the moles of the excess reagent on top and the moles of the element/compound that you were solving for on the bottom. Then you multiply that by the molar mass of the excess reagent. Finally you take the starting mass of the excess reagent subtracted by the number you just found. VOILA! You are now an expert! :)

Helpful links below!
STOICHIOMETRY - Limiting Reactant & Excess Reactant Video
Introduction to Limiting Reactant and Excess Reactant
Finding Limiting Reagent

Stoichiometry....what is it?!

The definition of Stoichiometry is the relationship between the relative quantities of substances taking part in a reaction or forming a compound, typically a ratio of whole integers. 

When I first saw this word on the board I couldn't even formulate a way to pronounce this! However, the first day of learning this was actually pretty good! It wasn't too confusing, for all it really involves are the atomic numbers, moles, and grams! Pretty basic! Plus Mrs. Frankenberg did a great job of explaining lots of examples on the board to help us memorize the process! I kinda love the beginning of this unit because it's pretty easy and doesn't require deep thinking that you would have to do in English! I think my favorite part of this is that the moles are just the coefficients of the reactant or product!! Super easy! 

Some helpful links below! 
What is Stoichimoetry?
Stoichiometry
Stoichiometry examples

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Night Before Exam

It's December 2 and today is my birthday. I'm spending over half of my night studying for this test.  I'm studying every study material I have. I'm practicing every problem. I'm looking at videos and rereading all of my notes. I'm just trying every possible thing to do in order to study. Net Ionic equations for double replacement is super easy and I feel good about it because you just switch cations with anions. However net ionic equations for everything else just confuse me a little bit. Synthesis, decomp, single replacement, and combustion are redox reactions, for you need to use the oxidation rules. If there are two nonmetals then you have to look at the periodic table to see whos is on top of each other and the element on top is stronger than the element on the bottom. Acid and Base always produce water. A strong base are group 1 and 2 elements on the periodic table.  A strong base has 2 or more oxygen's outweighing the hydrogen's. Also HBr and HCl are strong acids. Strong base/acids break apart in reactions completely. Today I did a rundown with all the rules that apply to every type of equation. I just hope all of my efforts pay off tomorrow!!!!!

Redox Lab

Today we did a REALLY cool lab! We put all of these metals into this little plate thing and put different solutions to mix with it! I think my favorite one was the calcium and copper (II) sulfate one! The reaction started bubbling then all of a sudden smoke started coming out from it and it was sizzling! How cool?! It then turned into a blue solid. After it cooled it started to expand a little to where we could see the inisde. What was really cool was that it was blue on the outside and a perfect snow white color on the inside! Another reaction happened simular to this but it was a brown solid but it didn't expand and crack like the blue one. Did anyone have a favorite reaction in the lab?