Take sample of Zinc Iodide and dissolve in solution. Then, take the battery, with exposed wire tips attached, and place the tips into the solution. In about 1-2 minutes, there should be a red-brown color coming out of one of the wires, and a dark substance depositing on the other wire, these should iodine and zinc respectively. 2. What are the identities of the substances found after electrolysis and heating?
Aim To compare the reactivity of various metals by observing their reaction with hydrochloric acid Hypothesis That the all the metals will produce foam and a pop. Variables Independent – Magnesium, Aluminium, Zinc, Copper Dependent – Detergent, Hydrochloric Acid Controlled – Size of the metals, amount of detergent and hydrochloric acid Materials 2 M hydrochloric acid Detergent 10 x test tubes and test tube rack and 5 rubber stoppers 0.5 cm pieces of magnesium, aluminium, zinc and copper 2 cm pieces of magnesium, aluminium, zinc and copper Steel wool Ruler Timer Bench mat Matches and birthday candle Marking pen Safety Remember to wear safety glasses and protective gloves when you do this experiment. 2 M HCl is corrosive. Wash with plenty of water should you get any on your skin or in your eyes. Method Part 1 1 Clean the surface of the 0.5cm piece of magnesium with a piece of steel wool 2 Place the magnesium into a test tube 3 Add three drops of detergent to the test tube 4 Add 2 cm of hydrochloric acid to the test tube.
The carbon rod is surrounded by a layer of manganese dioxide (MnO2), and a thick paste of ammonium chloride (NH4Cl) and zinc chloride (ZnCl2), which serves as an electrolyte. The oxidation reaction that takes place on the zinc casing is: Zn(s)→Zn+2+2e- While the reduction reaction that takes place on the carbon rod is: 2MnO2+2H+(aq)+2e-→Mn2O3(s)+H2O(l) The overall reaction is: Zn(s)+2MnO2+2NH4+(s)→Mn2O3(s)+Zn(NH3)22+(aq)+H2O(l) The standard dry cell contains 1.5V. The reactions present in dry cells continue until they run out of a reactant (the anode or cathode). However, there are cells that can be recharged, as the redox reaction can be reversed in order to regenerate the original reactants. Some examples of these batteries include lithium batteries and car batteries.
3. Light a candle that is secured in a candle holder. Use tongs to hold the aluminum with sugar in it over the flame; record observations. Sodium Carbonate and Hydrochloric Acid 1. Add a small amount of sodium carbonate to a beaker.
The Symbol Origin is from the Latin word 'aurum' meaning gold. Argentina was named for this precious metal.Facts about the Classification of the Element Gold Gold is classified as a "Transition Metal" which are located in Groups 3 - 12 of the Periodic Table. An Element classified as a Transition Metals is ductile, malleable, and able to conduct electricity and heat. Brief Facts about the Discovery and History of the Element Gold Gold was discovered in Ancient times and used by the ancient South Americans, Asians, Egyptians, Greeks, Romans and Chinese. It is mentioned in the Bible.
They go in order of the rainbow; red being the weakest and violet being the strongest. PURPOSE: The purpose of this experiment is to burn atoms of a metal using a flame burner to see how much energy a photon releases by the color of light emitted. Also by observing the photon; the ability to specify an unknown substance will be available. PROCUDURE: Seven well plates were obtained and labeled with the name of the known substances. In each well plate place a small amount of known substances into the well plate.
Radiographic film on the opposite side of the source is exposed when it is struck by radiation passing through the objects being tested. More radiation will pass through if there are cracks, breaks, or other flaws in the metal parts and will be recorded on the film. By studying the film, structural problems can be detected. Co-60 is used because it is an emitter of gamma rays which will penetrate metal parts. Co-60 has a half-life of 5.3 years and can be used in a chemically inert form held inside a sealed container.
6. Is it possible to light a candle without touching the flame directly to the wick? Why or why not? Materials • candle • matches • safety goggles • lab handout & pen • ruler • watch glass • 400 mL beaker • CO2 indicator solution (limewater) • 50 mL beaker (for indicator) Procedure My lab partner and I performed a series of experiments to investigate the chemistry of the burning of a candle. The teacher provided the following chemical equation to describe the burning, or combustion, in the candle: Hydrocarbon fuel + O2 ( CO2 + H2O The candle we used was a small, white emergency candle about 3.5 cm tall.
54Cr 24 g. 52Cr 24 f. e. 14C 6 d. 50Cr 24 c. 12C 6 b. 63Cu 29 a. 17O 8 Copyright © Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc. Chemistry: Matter and Change • Chapter 4 Mass contribution ( ؍mass)(percent abundance) For 27X: (27.977 amu)(92.23%) 08.52 ؍amu For 28X: (28.976 amu)(4.67%) 53.1 ؍amu For 29X: (29.974 amu)(3.10%) 929.0 ؍amu Atomic mass of X 08.52 ؍amu ؉ 1.35 amu ؉ 0.929 amu 80.82 ؍amu The element is silicon. Mass (amu) Isotope element. Show all your work.
Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid to manganese(IV) oxide in the following reaction: MnO2(s) + 4HCl(aq) ( MnCl2(aq) + 2H2O(l) + Cl2(g) a. Calculate the mass of MnO2 needed to produce 25.0 g Of Cl2 ans: 30.7 g MnO2 b. What mass of MnCl2 is produced when 0.091 g of C12 is generated? ans: 0.16 g MnCl2 1. How many moles of ammonium sulfate can be made from the reaction of 30.0 mol of NH3 with H2SO4 according to the following equation: ans.