course that covers fundamental concepts of chemistry‚ including measurements‚ states of matter‚ atomic theory and structure‚ chemical bonding‚ properties of matter‚ solutions‚ acids and bases‚ gases‚ intermolecular forces‚ chemical reactions‚ stoichiometry‚ and thermochemistry. Attendance: Attendance at all lecture and laboratory sessions is mandatory. Students will be dropped from course for excessive absences without valid excuses. Also‚ you are expected to be on time everyday. Grading:
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Chemistry 2202 Review Final Exam Chapter 2: The Mole 1. Isotope – atoms of an element that have the same number of protons but different numbers of neutrons. Ex. The three forms of oxygen are called oxygen-16‚ oxygen-17‚ and oxygen-18. They all have 8 electrons and are written as 16/8 O (8 protons + 8 neutrons)‚ 17/8 O (8 protons + 9 neutrons)‚ and 18/8 O (8 protons + 10 neutrons). 2. 3. Mass Number – the sum of the protons and neutrons in the nucleus of one atom of a particular
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liquids by vacuum filtration and drying solids are familiarized with. Introduction The reaction of sodium benzoate and hydrochloric acid is a typical phenomenon of hydrolysis reaction which conforms to the principles of acid-base chemistry and stoichiometry. In a typical hydrolysis reaction‚ when a salt dissolves in water‚ the salt dissociates to its constituent anions and cations (benzoate and sodium ions respectively). Also‚ when strong acids like hydrochloric acid dissolves in water‚ chloride ions
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Solubility and Stoichiometry I. Introduction The first purpose of this experiment is to apply solubility rules to choose two of eight given reactants to do a precipitation reaction. The second purpose is to use stoichiometry to calculate how much of a reactant will be used in a precipitation reaction‚ assuming that the amount of product is given‚ and to figure out the actual yield vs. the theoretical yield and to calculate the percent yield. The other purpose of this experiment is to practice the
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Mass % Determination of empirical formula and molecular formula Combustion analysis Balancing equations Chapter 4 Limiting reactant Mole to mole conversion from reaction stoichiometry Theoretical yield‚ Percent yield‚ Actual yield Solution concentration (molarity) M = n/V ‚ V always in L M1V1=M2V2 ( dilution calculations) Stoichiometry of reactions in solutions M1V1=M2V2 ( dilution calculations) Ionic reactions (formula unit equation‚ complete ionic and net ionic equation). Solubility rule Types of
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Introduction: During this lab‚ we found the excess reactant and limiting reactant between Aluminum and Copper (ll) Chloride. Using stoichiometry‚ we were able to make predictions. Through the reaction 2Al + 2CuCl₂ → 3Cu + 2AlCl₃ we carried out this experiment and determined that the limiting reactant was CuCl₂ and that the aluminum was in excess. We also determined the percentage yield of copper. Purpose: The purpose of this experiment was to determine the limiting reactant and percentage yield
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Finally we weighed the filter paper and recorded the mass in our data table. Our result for this lab was that both total product and the mass of the total reactants was 2.71g we had a 2.5 difference. This shows that we did not validate the stoichiometry of mass. That we lose moles or it’s mass. The physical changes in this lab were that the blue copper rocks changed to blue liquid. The Error we faced in this lab was that copper residue did not end up in the filter paper. II. Objective
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of solubility and the formation of a precipitate. The Experiment and Observation: Weigh out your 1.0g of CaCl2-2H20 and put it into the 100mL beaker‚ add your 25mL of distilled water and stir to form the calcium chloride solution. Next‚ use stoichiometry to determine how much Na2CO3 and put it into a small paper cup. Then add the 25mL of distilled water to make the sodium carbonate solution. Mix the two solutions in the beaker and a precipitate of calcium carbonate will form instantly. Next‚ set
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Experiment 4 SOLUTION STOICHIOMETRY ACID-BASE TITRATIONS Determination of the Percent Acetic Acid in Vinegar Objectives: (1) To introduce and use the concept of solution stoichiometry (2) To specifically use solution stoichiometry to determine the percent of acetic acid in vinegar. (3) To prepare a standard solution by the method of titration. Consider the following balanced chemical equations: (1) HCl + NaOH ------> NaCl + HOH (2) H2SO4
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! Name: Laura Romero ! 5.04H: Gas Stoichiometry Lab Worksheet Data and Observations: Present all relevant data in a data table below. Include an observations section for any observations that you made during the lab. (5 points) Data Table Mass of magnesium strip (grams) 0.032 g Volume of gas collected (mL) 30mL Barometric pressure (atm) 1.1 atm Room Temperature (°C) 22 °C Vapor pressure of the water (torr) 19.8 torr ! ! Calculations: ! 1. Write the
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