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| Hey what's up everybody... I'm exciyed because I'm typing this entry on my sidekick yo
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| Cathryn Mattimore
12/12/05
Period 3
Calculating the Amount of Copper Produced from a Single Replacement Reaction
When copper II sulfate reacts with iron, what will the final mole ratio be and how much copper will be produced?
Procedure:
o Mass a clean dry 100 ml beaker
o Mass out 12.5 grams of copper II sulfate into the 100 ml beaker that has already been massed
o Measure 50.0 mL of deionized water and add the water to the beaker containing the massed copper II sulfate
o Using a piece of weighing paper, mass out 2.24 grams of iron fillings. Set aside.
o Use a hot plate to heat the beaker containing copper II sulfate and water. Be sure to not let this boil.
o To help the crystals dissolve stir with a glass stirring rod.
o When the crystals are completely dissolved, stop heating.
o While stirring, carefully mass the iron fillings to the hot solution. When the iron has been added, let the beaker sit for ten minuets. Stir occasionally and be sure to make observations.
o When the ten minuets are up decant the liquid into a 250 mL beaker.
o To wash the solid, add 10 mL of dienoized water and then decant the liquid.
o Repeat this step at least 2 more times
o Spread the product out of the bottom and let it dry over night
o Determine the mass of the product the next day.
o Rinse the decanted liquid with a lot of water, and turn in the copper.
Data:
o The beaker containing the water and the copper sulfate was a aqua blue. When the mixture was heated the crystals dissolved
o When the iron fillings were added to the copper sulfate, the solution turned a dark green color indicating that a chemical reaction occurred.
o Also there were red clumps that gathered at the bottom of the beaker.
Analysis:
o Mass of empty beaker- 51.33g
o Mass of iron fillings- 2.24g
o Mass of beaker and dry copper metal- 53.68g
o Mass of copper produced- 2.33g
53.68g- 51.33g = 2.33g
o Number of moles of copper produced- .04 moles
2.33g/ 63.55= .04 moles
o Number of moles iron reacted-
2.24/ 58.85= .04
o The mole ratios of iron reacted with copper- 1 to 1
Equations:
Word Equation:
o Iron + Copper II Sulfate ànd Iron II Sulfate and Copper
Formula
o Fe+ CuSO4 à FeSO4+ Cu
o Percent yield- 91.73%
o Percent Error- 8.27%
Conclusion:
Through this experiment, by combining copper II sulfate and iron, a single replacement reaction occurred leaving the product of copper and iron II sulfate. The total amount of copper that was produced was 2.33g. The mole ratio of iron reacted and copper produced was 1 to 1. In conclusion, iron fillings reacted with copper II sulfate produces copper medal.
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| Cathryn Mattimore
December 7, 2005
Period 3
Chapter 8 Self Directed
Vocabulary
1. Alpha radiation- rapidly moving helium ions that are positively charged.
2. Anion- negative ion.
3. Anode- positive electrode and site of oxidation in voltaic cell.
4. Atomic number- number of protons in the nucleus of an atom of a given element.
5. Beta radiation- electrons emitted at very high speed, often approaching the speed of light.
6. Cathode- negative electrode and site of reduction in a voltaic cell.
7. Cathode ray tube- (CRT) vacuum tube used to direct cathode rays onto a fluorescent screen.
8. Cation- positive ion.
9. Electrode- conductor used to establish electrical contact in a circuit.
10. Electron- elementary particle with negative electric charge; name coined from the British physicist G.J. Stoney.
11. Fluorescent- description of material that glows when it absorbs certain kinds of energy such as electrons
12. Gamma radiation- electromagnetic energy waves that are similar to, but more energetic then X- Rays.
13. Isotopes- atoms of the same element that contain different number of neutrons, consequently having different atomic masses.
14. Mass number- total number of protons and neutrons in an atom’s nucleus.
15. Neutron- uncharged particle found in the nucleus of an atom.
16. Nucleus- dense, positively charged center of an atom
17. Proton- positively charged particle found in all atoms
18. Radiation- term for energy emitted from a source and traveling through space.
19. Radioactivity- spontaneous emission of radiation from the nucleus of an atom.
Addendum
1. A) By using a CRT and positioning a positive plate and a negative plate above and below the tube, Thomson could prove the electrons to be negative because the ray of electrons sloped up towards the positive plates.
B) Thomson did an experiment in which he used different metals as electrodes and different gases. The results were always the same. When he weighed the electrodes they were no less in mass, proving that it wasn’t true that atoms were coming off. However, something in the atom has a negative charge (the electrons) and all atoms had them. It proved that atoms were not invisible.
2. The charge in the nucleus of every atom is positive because the nucleus consists of protons, which have a positive charge, and neutrons, which have no charge. This would cause the nucleus to be positive.
3. The atoms are electrically neutral because it consists of protons, which have a charge of +1, neutrons with a charge of 0 (neutral) and electrons with a charge of –1. Assuming there is the same number of protons as there are electrons the negative and positive charges cancel each other out leaving the atom neutral.
4. The atomic number is the number of protons in the nucleus of an element and the atomic mass is the mass of an atom of the element in atomic mass units (amu’s).
5. Isotopes occur when the element has different has a different number of neutrons and a different atomic mass.
6. No, Dalton’s atomic theory should not be taken as a criticism to Dalton as a scientist because although he was incorrect in some areas of his model, he still provided a platform for other scientists to work from.
7. Although atoms can be broken into smaller things like protons, electrons, and neutrons, the atom is still the smallest thing that retains all the properties of an element. Therefore the atom is the basic building block of matter.
8. A) 2.7948
B) 54.0956
C) 43.0974
D) 107.224
Total: 207.2118
9. A)92.90%
B) 99.89%
C) .0001%
10. A) Electron
B) Proton
C) Brick
Pages 286- 291
1. The beam of calcium- 40 ions would be deflected more because it has a lower mass in comparison with the calcium- 42. The lesser the mass is the greater the deflection will be.
2. If all the ions had the same velocity the sulfur- 32 ions with two extra electrons would be deflected more because it has a greater charge and is more attracted to the magnet then the sulfur – 32 with one extra electron.
3. Assuming that the sodium and potassium ions have constant velocities and charges a magnet would bend the sodium more because it has a lesser mass then the potassium.
4. Neither gamma rays nor a beam of neutrons will be attracted to a magnet because they bath have no charge and gamma rays have no mass.
8. Thomson came after Dalton and he therefore was able to use information discovered by past scientist, like Dalton and Crooke to help him prove that the beam of particles was charged. His model was now the plum pudding model rather then Dalton’s cue ball model.
9. Dalton saw that elements would always combine in the same percent by mass each time the compound was formed. The law of definite proportions comes into play. For example when water is formed (H20) you can set up a proportion using each elements mass.
The same idea can be applied to all compounds, like sodium chloride.
13. A neutral atom can become a charge of 2- by adding two electrons.
14. A neutral calcium ion can become a 2+ ion by losing 2 electrons, having 2 more protons then there are electrons.
15. The difference between a neutral sodium atom and a Na+ ion is that the ion has one less electron then the neutral atom.
17. A) Anion and gained one electron
B) Cation and lost two electrons
18. A) Gamma
B) Beta
C) Gamma
D) Alpha
E) Gamma
F) Beta
19. Alpha has a positive charge and a mass of 4.003g, Beta has a negative charge and a mass of 9.11 x 10^-28, and gamma has no mass and no charge.
25. The problem with Rutherford’s model was that he thought the electrons moved at high speeds around the nucleus. According to the laws of physics known at the time orbiting electrons should radiate light, causing them to lose energy and to spiral into the nucleus. With this model Rutherford is contradicting the laws of physics.
30. Calcium’s five different isotopes differ because they have the same atomic mass and they have a different number of neutrons. The five isotopes of calcium are alike because they have 20 protons, 20 electrons and an atomic number of 20.
32. The atomic number is 15 the atomic weight is 31 and the symbol if P.
37.
Isotope Atomic number Mass number Symbol
Molybdenum 42 92 96/ 42 MO
Technetium 43 96 98/ 43 TC
Manganese 25 55 55/ 25 MN
42.
Symbol Kr Mn U P
Atomic number 36 25 92 15
Mass number 84 55 235 32
# of protons 36 25 92 15
# of neutrons 48 30 143 17
# of electrons 36 25 92 15
46. A) 3 protons, 2 electrons, 4 neutrons
D) 15 protons, 18 electrons, 16 neutrons
52. 2.69 x 10^16 molecules
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