Monday, February 13, 2012
Book Problems!!
Yes that is me with all my beautifully designed problem cards I did for Mr. Ludwig! Mr. Ludwig told me it would be a lot of extra work to put all these problems on individual little cards, but it actually kept my work organized and help me keep the problem clean and accurate. These problems came from chapter 11 in our Glenco Chemistry book. The problems are 42-57 and 60 to 64 I do believe. These problems have covered subjects that included the empirical formula, moles, and the molecular formula.
Tuesday, February 7, 2012
Element Identification
Element Identification
So in this lab we had a procedure on google docs, provided by none other then Mr. Ludwig and his handy dandy technology equipment! We were to calculate the atomic mass of different elements in order to define which was which!
Here is how we did it…
Element A
.163mol / 6.52g × 6.02 × 10²³ / 1 mole = 6.52/.163 = 40
Element = Calcium
Element B
.91mol / 24.51g × 6.02 × 10²³ / 1 mole = 24.51/.91 = 26.93
Element = Aluminum
Element C
.160mol / 9.45g × 6.02 × 10²³ / 1 mole = 9.45/.160 = 59.06
Element = Cobalt
Element D
.268mol / 53.87g × 6.02 × 10²³ / 1 mole = 53.87/.258 = 208.79
Element = Bismuth
Element E
.220mol / 14.25g × 6.02 × 10²³ / 1 mole = 14.25/.220 = 64.77
Element = Zinc
Element F
.756mol / 49.25g × 6.02 × 10²³ / 1 mole = 49.25/.756 = 65.145
Element = Zinc
Element G
.492mol / 28.65g × 6.02 × 10²³ / 1 mole = 28.65/.492 = 58.23
Element = Nickel
Element H
.430mol / 89.11g × 6.02 × 10²³ / 1 mole = 89.11/.430 = 207.2
Element = Lead
Element I
.381mol / 21.28g × 6.02 × 10²³ / 1 mole = 21.28/.381 = 55.85
Element = Iron
Element J
.259mol / 30.66g × 6.02 × 10²³ / 1 mole = 30.66/.259 = 118.37
Element = Tin
Popcorn Lab!
Pop, Pop, POPCORN!
Procedure:
1. Add enough vegetable oil to cover the bottom of the beaker. Make a tight cover for the beaker for the aluminum foil. Weigh the beaker as it is and record the weight
2. Add 25-30 kernels of popcorn to the beaker and replace the lid. Weight the beaker again, with the popcorn in it
3. Poke several holes in the aluminum foil and place it on the ring stand over the Bunsen Burner
4. When the popcorn is finished popping, remove the heat and carefully take off the aluminum cover
5. Let the beaker stand until it is cool. Once it has cooled, weigh the beaker with the popped corn and the cover on
!!!!RECORD THE DATA!!!!
I did this lab with Mr. Steven and our results were…
| Beaker and Oil | 192 Grams |
| Beaker, Oil, and Corn | 198.5 Grams |
| Beaker, Oil, and POPcorn | 197.5 Grams |
Conclusion:
Well overall in this lab I wasn’t here for the first day to get all the yummy popcorn we could actually eat, but hey that’s okay! However I did learn that popcorn loses water mass as the kernels are heated up and reach the point of popping. That’s why when you place a bag of popcorn in the microwave it is always more heavy going in then it does coming out. Water mass is what keeps the kernels from burning when they are being heated to pop. So results showed that our popcorn lost around about 1% give or take of its water content!
Baking Soda Lab!!!
Baking Soda Lab
Purpose: To find the experimental mole ratio of the reaction of baking soda with vinegar
Background: Baking soda is pure sodium hydrogen carbonate (NaHCO₃) Vinegar is an aqueous solution of acetic acid (HC₂H₃O₂)
Balanced Equation: NaC₂H₃O₂ + HC₂H₃O₂ à CO₂ + H₂O + NaC₂H₃O₂
Mole Ratio of Balanced Equation: 1 to 1
Materials: 20ml vinegar in a large pipette
Balance
100ml beaker
1 Gram Baking Soda
Procedure:
1. Get a large plastic pipette filled with vinegar. Measure the mass of the pipette and record the mass
2. Measure the mass of an empty, clean 00 ml beaker
3. Transfer about 1 gram of baking soda to the beaker. Record the exact mass of the beaker with the powder
4. Add vinegar, from the pipette, to the beaker. Swirl the contents and observe the reaction. Continue to add vinegar until no more bubbles are produced. This will take a while so be patient and pay close attention to the reaction
5. Find the mass of the left-over vinegar in the pipette and record. Subtract the original mass of this pipette to find the mass of the vinegar used in the reaction
| Initial Mass of Pipette in Grams | 1.36 Grams |
| Final Mass of Pipette at End of Reaction | 2.52 Grams |
| Net Mass of Vinegar Used in Reaction | 9.81 Grams |
| Mass of Empty Beaker | 113.73 Grams |
| Mass of Beaker and Baking Soda | 114.73 Grams |
| Net Mass of Baking Soda | 1 Gram |
Conclusion Questions:
1. Calculate the moles of sodium hydrogen carbonate used from the net mass of the baking soda.
1gNaHCO₃ × 1 mole / 81g NaHCO₃ = .0123 moles
2. There are 5 grams of acetic acid per 100 grams of vinegar. Calculate the grams of acetic acid added to the beaker for the reaction.
5% of 9.81 = .49 grams of acetic acid
3. Calculate the moles of acetic acid used in the reaction.
.49gHC₂H₃O₂ × 1 mole / 60g HC₂H₃O₂ = .0081 moles
4. Compare the moles of sodium hydrogen carbonate with the moles of acetic acid used in this experiment. Find the nearest whole number ration between the two values.
Experimental Ratio: 2 to 3
5. The ratio calculated above is your experiment mole ratio. Is this mole ration the same as the mole ratio in the balance equation?
No, due to rounding errors along with weighing errors resulted in the chance in the results.
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