We determined that the mass of zinc necessary to completely react with the copper (II) ions in the solution was 1.308g. We added an excess of 0.050 to make sure the copper completely reacted. 1.358g of zinc was then added to the solution. The solution with the zinc was heated and stirred until it was colorless, showing that the reaction was done. Hydrochloric acid was then added to the solution until the bubbles stopped in order to completely get rid of all of the zinc.
Show ALL your work. Use the given specific heat capacity values below to calculate the percent error of the experimental specific heat capacity that you determined in Part I of the lab. Known specific heat values — Iron: 0.444 J/g°C; Zinc: 0.390 J/g°C; Copper: 0.385 J/g°C, Aluminum: 0.900 J/g°C Percent Error == | experimental - actual value | / actual value x 100 % Using the specific heat capacity value that you determined in Part II of the lab, what is the most probable identity of the unknown metal that you examined? Please explain your reasoning in complete sentences. I believe the most probable identity of the metal is Silver because it is the closest to the experimental heat value.
By recording the amount of silver nitrate (AgNO3) is used, the amount of the chloride used is figured. An indicator is used to help determine when the reaction is complete. The indicator used in this experiment is potassium chromate (K2CrO4). The recorded volume of silver nitrate (AgNO3) used is then used to determine the molarity of the silver chloride (AgCl) created. Moles of AgCl = (Volume of AgNO3 added) × (Molarity of AgNO3) Using the molarity of the silver chloride (AgCl) and the atomic weight of the chloride (35.4527), the weight of the chloride from the original unknown chloride salt sample.
Sodium Hydroxide + Hydrochloric Acid Sodium Chloride + Water NaOH(aq) + HClaq → NaCl(aq) + H2O(l) Variables Independent The independent variable of the experiment was the amount of sodium hydroxide that we added to the acid. To keep the variable controlled we would measure 1 ml of the sodium hydroxide and pouring that to the hydrochloric acid. Dependent The dependent variables of the experiment were the temperature and the pH number of the mixture. To control the pH and temperature use the electronic probe and data logger. Controlled The controlled variables of the experiment were: A.
(4 points) q = m × c × Δt Given: q=? m = 34.720g c = 4.18 j/(g x °C) Δt = 41.6°C - 25.2°C = 16.4°C q = (34.720g) (4.18 j/(g x °C) (16.4°C) q = 2380.13j You are trying to figure out the energy change of the water which is the surroundings in the lab. To do that you must take the mass of the metal, which for me was Aluminum, and multiply it by the heat capacity of the water, which was given, then multiply that by the change in temperature, which is the final temperature of the mixture
Year 11 Chemistry Electrochemical Cells Purpose To determine the order of reactivity for the metals copper, iron, lead and zinc using the least amount of electrochemical cells as possible. Materials List • Four 100ml beakers • 4 strips of filter paper approximately 15cm in length • Voltmeter • Sodium Chloride solution at 10% concentration • Zinc, Copper, Lead and Iron metal strips (approximately 10 cm) • 50 ml of Copper sulphate, Zinc sulphate, Lead nitrate and Iron nitrate solutions • Scissors Procedure - Place the 50ml solution of zinc sulphate in a 100ml beaker, and 50ml solution of copper sulphate in a different 100ml beaker. Place the zinc metal strip in the zinc sulphate beaker and the copper metal strip with the copper sulphate beaker.
- 1 Spectrophotometer. Method to obtain solutions: - Weigh 0.25g of Cu powder in a beaker. - Under fuming cupboard add 1 cm^3 of Nitric Acid in the same beaker. - Pour the Copper Nitrate solution into the 250 cm^3 volumetric flask and dilute it with water until it reaches the line. - Using a pipette pour 5cc, 10cc, 15cc and 20cc of the solution into different volumetric flasks each of 100 cm^3 volume and dilute them until the line mark and
Determination of Copper Metal Ions Through Reactions with Zinc Aim: The aim of this experiment is to determine which of the common copper ions, Cu+1 and Cu+2, is present in each of two unknown copper compounds, and whether or not the copper compounds contain the same copper ion. Nomenclature: Light blue substance: LB Dark blue substance: DB Preliminary Calculations: Identify the available test metal with the highest ionization energy. The available test metal with the highest ionization energy is Zinc. Because Zinc has the highest ionization energy (904) compared to Magnesium (736), and Aluminium (578), Zinc will be used in this experiment. Create reactions with anion placeholders for copper compound and Zinc.
The more active the metal the more basic it’s saturated hydroxide solution. The sulfate compounds of alkaline earth metals show decreasing solubilites as you go down a group. This characteristic is used as a means of separating and identifying metallic ions in a group. Carbonates are pretty insoluble. You will observe in this experiment some of the characteristics of the alkaline earth metals discussed here and will write balanced equations for all reactions.
The Formula of Magnesium Oxide Aim:- To find the empirical formula of magnesium oxide by burning a weighted amount of magnesium ribbon in air. Data collection, processing and presentation:- Qualitative Data: Before the magnesium strip was put in the crucible to react with oxygen it was a silverly shiny solid. when the magnesium started reacting with oxygen it changed color, but all that was seen was a white flash. As the reaction continued a white solid powder started forming around the magnesium and was soon starting to spread out all over the crucible. The ending result was some left over magnesium, that at this point was white, and the white solid powder that covered the crucible on all sides.