In force and spark compositions, potassium nitrate, sulfur, and finely ground charcoal are used, with additional ingredients that produce various types of sparks. In flame compositions, such as the stars that shoot out of rockets, potassium nitrate, salts of antimony, and sulfur maybe be used. For colored fire, potassium chlorate or potassium perchlorate is combined with a metal salt that determines the color. Inside each firework are small packets filled with chemicals, mainly metal salts and metal oxides, which react to produce an array of colors. When heated, the atoms of each element in the mix absorb energy causing its electrons to rearrange from their lowest energy state to a higher excited state.
obseRvations The color of the flame is expected to be as follows: Metallic ion Flame color Sodium Na+ Bright Orange Strontium Sr2+ Red/Orange Potassium K+ Pink Barium Ba2+ Yellow Copper Cu2+ Yellow/Green Lithium Li+ Red Calcium Ca2+ Deep Orange Unknown Red-Lithium Questions A. All chemical used in this test are binary compounds. What portion of the periodic table is responsible for the color observed? Groups 1&2 (Alkalil metals) B. In cooking over an open flame, a yellow flame is often observed when some food is spilled into the flame?
Determining the Chemical Formula of a Hydrate Purpose: Find the molecular formula of the hydrate of Copper (II) Sulfate. Materials: * 400 mL beaker * Tongs * Scoopula * Electronic Balance * Glass Rod * Hot Pad * 3 g hydrated copper(II) sulphate * Eye Protection Hypothesis: This lab will demonstrate a dehydration reaction. When the beaker containing hydrated copper (II) sulphate is heated, the water will evaporate, causing the color to change from blue to white, and the mass to decrease. Procedure: 1. Measure & record mass of beaker 2.
6.) In step 6 we added 4 grams of zinc to the solution. When we added the zinc it immediately began to fizz followed by the formation or red clay like solid that floated on the surface of the solution. Reaction 1: Copper metal To Copper Nitrate Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Cu + 4H1+ + 4NO31- Cu2+ + 2NO31- + 2NO2 + 2H2O Cu + 4H1+ + 2NO31- Cu2+ + 2NO2 + 2H2O Reaction 2: Copper Nitrate to Copper Hydroxide Cu(NO3)2(aq) + 2NaOH(aq) 2NaNO3(aq) + Cu(OH)2(s) Cu2+ + 2(NO3)1- + 2Na1+ + 2OH1- 2Na1+ + 2NO31- + Cu(OH)2 Cu2+ + 2OH1- Cu(OH)2 Reaction 3: Copper hydroxide to copper oxide Cu(OH)2(s) + heat CuO(s) + H2O(g) Reaction 4: Copper oxide to copper sulfate CuO(s) + H2SO4(aq) CuSO4(aq) H2O(l) CuO + 2H1+ + SO42- Cu2+ +SO42- + H2O CuO + 2H1+ Cu2+ + H2O Reaction 5: Copper sulfate to copper metal
Safety Considerations: Always have safety goggles covering your eyes, do not inhale the fumes of chemicals used. Also to not eat or drink chemicals used in this lab. Procedure:Begin by assembling the calorimeter using styrofoam cups. Poke a hole in the lid. Record the initial temperature of the liquid in the calorimeter.
One serious blunder could have been not paying attention. Because we had to record the amount of time the Mg strip dissolved, we had to keep a close eye on the reaction. One thing that could have affected this was talking to others around you, or trying to multitask. Generally speaking, systematic and random errors did not have a great effect on my data and results. However, if the blunder were true, my data would have been completely wrong resulting in an incorrect graph and rate law for magnesium.
The mixture was decanted again in to the same beaker. Next, we added boiling chips to the liquid and evaporated the solvent over the hot plates under the hood. After the solvent was evaporated and the flask was cooled, we used a spatula to remove a small amount of the crude product and took its melting point. We determined the melting point range of the sample to be 43.0-46.0 degrees Celcius.The crude product was yellow colored when it was warm and orange in color when cooled and sticky. We then recrystallized our sample using 5 ml of warm acetone that was heated on a hot plate under a hood.
Observations: * Solution turns green and bubbles * Warm to the touch * Brown gas produced * Copper Dissolves Reaction 2: Copper (II) Nitrate with Sodium Hydroxide Cu(NO3)2(aq) + 2NaOH(aq) Cu(OH)2(s) + 2NaNO3(aq) Net ionic: Cu2+(aq) + 2OH-(aq) Cu(OH)2(s) Type of Reaction: Precipitate Reaction Observations: * With addition of water, the solution becomes blue, thick, and slime-like * When added to litmus paper, paper turns dark blue * Dark blue shows that the solution is basic Reaction 3: Heating Copper Cu(OH)2(s) CuO(s) + H2O(l) Net ionic: Cu(OH)2(s) CuO(s) + H2O(g) Type of Reaction: Redox Reaction: Cu is oxidized from 2- to 2+. The reducing agent is Cu(OH)3 Observations: * While heating and stirring, solution turns greyish blue, then becomes black * Cool water mixes, solution settles to the bottom * *NOT ALL WATER WAS POURED OFF Reaction 4: Copper (II) Oxide with Sulfuric Acid CuO(s) + H2SO4(aq) CuSO4(aq) +
Effects of mustard agents C. Protection against mustard agents II. Mustard agents compared to other agents used on the battlefield A. Choking agents B. Nerve agents C. Other blister agents III. Use of mustard agents in war A. WW I B. WWII and Italian-Ethiopian War C. The Yemen Civil War and The Iran-Iraq war IV. Conclusion A man named Frederick Guthrie in 1860 first synthesized mustard gas. During his research, he reacted ethylene with (chlorine) CL2, and noticed the toxic effects it had on his own skin.
• Created Data Table using the recorded information from each test. Data Table 1: Reactions Well #/ Question Chemicals Reaction A NaHCO3 and HCI - C02 No Physical reaction when Bleach was added. Over white paper I could see somewhat of a difference in chemicals but not over the dark paper. B HCI and BTB When HCI & BTB were added together the solution turned a bright yellow. Once the bleach was added the solution turned back to clear.