Determining the Stoichiometry of Chemical Reactions Objective In this lab we took Fe(NO3)3 and NaOH and mixed 7 different mole ratios in graduated cylinders to determine what the mole ratio is. We also did the same thing with solutions of CuCl2 and Na3PO4. We determine the mole ratios by graphing the volume of reactant #1 vs. volume of precipitate for each reaction. Data Part 1.) Cylinder 1 2 3 4 5 6 7 Fe(NO3)3‚ 0.1 M‚ ml 5 10 12 15 17 20 24 NaOH‚ 0.1 M‚ ml 55 50 48 45
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Millimole – 1mmol = 10-3 mol 3. Molar mass – mass in grams of one mole of a substance. Example 3-5 page 76 4.62 g Na3PO4 Molar Mass Na3PO4 = (22.9898 gNa X 3) + (30.9738 gP) + (15.9994 gO X4) = 163.9408 g per mol Na3PO4 Moles Na3PO4 = 4.62 g X 163.9408 g/ mol = 2.818 X 10-2 mol Na3PO4 Moles Na = 2.818 X 10-2 mol Na3PO4 X 3 mol Na / mol Na3PO4 = 8.45 X 10-2 mol Na Na+ ions = 8.45 X 10-2 mol Na X (6.022 X 1023) = 5.08 X 1022 ions C. Solutions and Their Concentrations
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insoluble in water. a. MgBr2 d. Sr(OH)2 b. PbI2 e. ZnSO4 c. (NH4)2CO3 5. (Brown 4.20 w/ additional) Predict whether each of the following compounds is soluble in water: a. AgI f. Sr(NO3)2 b. Na2CO3 g. CuSO4 c. BaCl2 h. CuCl2 d. Al(OH)3 g. PbS e. Zn(CH3COO)2 6. Complete the following double replacement (exchange ) reactions. Be sure to balance them. a. MgCl2 + Ba(NO3)2 → b. Al2(CrO4)3 + (NH4)2SO4 → c. K2SO4 + SrCl2 → d. FeCl3 + KOH → e. HCl +
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Calculations: Part I: Dehydration of Hydrated Copper Chloride)‚ which showed how much of the compound was copper chloride by mass. Since there are only two stable forms of copper chloride‚ we concluded that possible formulas would be either CuCl or CuCl2. Intending
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EXPERIMENT 2 Stoichiometry Introduction Stoichiometry is the study of the quantitative relationships in chemical reactions. By studying stoichiometry‚ you can calculate the quantity of reactants that will be consumed in a chemical reaction‚ and the amount of product produced. Consider the reaction of vinegar with baking soda. As you may know‚ this reaction produces carbon dioxide gas which bubbles out of the vinegar. But if you want to know how much gas would be produced from combining a teaspoon
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The data gathered and calculated in the experiment accurately portrayed the way the reactions would have taken place. The chloride analysis was a little bit off from other groups due to the fact that our AgCl was in clumps‚ creating less surface area‚ thus our product took longer to burn and may not have burned correctly compared to other groups; yet there are several experimental factors that could have caused us to have different results than other groups‚ i.e. different measurements for samples
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Chemistry Review (mid-term) 1. Use the equation for atomic mass to answer the following questions. (http://johnheilchem10.escuelacampoalegre.wikispaces.net/file/view/average+atomic+mass+calculations+-+3.pdf) 1. Argon has three naturally occurring isotopes: argon-36‚ argon-38‚ and argon-40. Based on argon’sreported atomic mass‚ which isotope do you think is the most abundant in nature? Explain. 2. Copper is made of two isotopes. Copper-63 is 69.17% abundant and it has a mass of 62.9296 amu.
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CHM138LL Lab 5 Stoichiometry Analysis of a Chemical Reaction Name: A. Data Tables Item Measured/Quantity Calculated Mass (in grams) Iron nails (before reaction) 7.75g 5.5g Iron nails (after reaction) Mass of iron consumed 2.25g Initial mass of filter paper (before filtration) 0.86g 3.52g 2.66g Mass of filter paper and solid product Mass of solid product Show work below for “mass of iron consumed” and “mass of solid formed” calculations: 7.75g-5.5g=2.25g 3.52g-
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Section 10.10 Balancing Oxidation–Reduction Equations ENERGY General Chemistry 2 (Chem 112) Return to TOC Copyright © Cengage Learning. All rights reserved 1 Section 10.10 Balancing Oxidation–Reduction Equations UNIT 1: ENERGY MODULE 1: ELECTROCHEMICAL ENERGY MODULE 2: NUCLEAR ENERGY MODULE 3: FUELS Return to TOC Copyright © Cengage Learning. All rights reserved 2 Section 10.9 Oxidation–Reduction Reactions Redox Reactions • Reactions in which one
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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