chloride and they form a solid precipitate. Then we poured it a funnel with a filter paper to get the solid precipitate. Purpose ● The purposed of the lab is to lets us student know if we know how calculate the percent yield of a double displacement reaction while using the grams that we get from our lab. Objectives ● We need to know the solid precipitate that had been formed in the
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Single Displacement Reaction The objective of this experiment was to observe evidence of a reaction and to determine the chemical equation‚ if there is a reaction. In order for a reaction to occur‚ a metal strip must have evidence of black or grey deposits on the surface of the metal once dipped into the solution. The reactivity of an element is related to its tendency to lose or gain electrons. Three metal strips that were used are copper‚ lead and zinc as well as the solutions of silver nitrate
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the concentration does not change any further for specific temperature and pressure. At any given temperature‚ the maximum amount of solute that dissolves in a fixed quantity of particular solvent determines the degree of solubility (Chang & Goldsby‚ 2014). For most ionic compounds‚ changes made to the temperature affect the
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Classifying Chemical Reactions Purpose: To observe and differentiate between the four different types of chemical reactions. Variables: The independent variables are the sodium chloride‚ sodium carbonate‚ magnesium‚copper‚ copper (11) sulfate‚ silver nitrate‚ oxygen‚ lead(11) nitrate‚ sodium carbonate‚ copper (11) sulfate pentahydrate. The dependent variables are the chemical reactions that are being looked for. For example decomposition‚ synthesis‚ single displacement or double displacement of compounds
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seconds for a reaction between copper (II) sulfate (CuSO_4) and zinc(Zn) using a temperature probe. Time/ s (± 1 s) Temperature / °C (± 0.05 °C) 0 27.9 30 25.9 60 25.9 90 25.8 120 25.8 150 48.7 180 57.6 210 61.1 240 62.7 270 63.5 300 62.8 330 61.3 360 59.3 390 58.9 420 57.7 450 56.5 480 55.2 510 54.2 540 52.6 570 51.9 600 51.1 Qualitative observations:- Table 2: table depicting the qualitative observations observed during the reaction between Copper (II) sulfate solutions (CuSO_4) and Zinc (Zn). Solution
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Chemical Reaction of copper compounds Introduction: In this experiment‚ the objective was to conduct a series of chemical reactions that contain copper or copper compounds. That is to say that the products of each chemical reaction were used in the next reaction. The process starts with a solid copper wire dissolved in nitric acid and the end product is copper powder. The product which was used from the previous reaction is the limiting. In the initial step‚ the solid copper is the limiting reactant
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Copper Sulphate Calibration Aim The objective of this experiment is to determine the unknown concentrations of solutions. Introduction With the use of absorption of light a spectrophotometer sends UV wavelengths through solutions to determine their concentrations. The light absorbed is measured as the atoms‚ molecules and ions absorb the wavelengths of light that the spectrophotometer gives off (Meah‚2013). The level of light transmitted defines the amount of light absorbed‚ for instance‚ the lower
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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy D. F. Nachman 6/23/2010 Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M sulfuric acid solution: Mg(s) + H2SO4(aq) →MgSO4(aq) + H2(g). We found the experimental molar enthalpy of reaction to be ΔH = –355 ± 17 kJ/mol at 0°C‚ 24% lower than the textbook value of ΔH° = –466.9 kJ/mol‚ reported at 25°C. Introduction Whether a chemical reaction occurs spontaneously or is driven by an outside force
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Step 1: Pb (NO3) 2 (aq) + CaCl2 (aq) PbCl2 (aq) + Ca (NO3) 2 (aq) (double displacement reaction) According to the solubility guidelines lead (II) chloride (PbCl2) is a possible precipitate. This is because even though most chlorides are soluble‚ lead chloride is considered insoluble (p.2‚ Lesson 17). Step 2: PbCl2 ↔ Pb2+ + 2Cl- Q = [Pb2+] [Cl-] 2 Step 3: Ksp = 1.2 x 10-5 (from table 17.1‚ p.5) Step 4: V2 = 20.0 mL (volume of Pb (NO3)2) + 45.0 mL (volume of CaCl2) = 65.0
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Chapter 1 Chemical Reactions and Equations Q.1. Why should magnesium ribbon be cleaned before burning in air ? Ans: Magnesium ribbon is a very reactive metal. When stored it reacts with oxygen to form a layer of magnesium oxide on its surface. This layer of magnesium oxide being a stable compound prevents further reaction of magnesium with oxygen. The magnesium is cleaned before burning in air to remove this layer so that the metal can be exposed to air properly. Q.2. Write the balanced
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