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    Energetics Practical

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    Energetics Practical 2: To Determine the Enthalpy Change of a Reaction Background Calcium Carbonate‚ CaCO₃‚ decomposes with heat to form CaO and CO₂. The objective of this practical was to determine the enthalpy change for this reaction by using an indirect method based upon the foundation of Hess’ Law. Both calcium oxide and calcium carbonate react readily with 2 mol/dm3. The reaction can be demonstrated as so: CaCO₃ (s) -> CaO(s) + CO₂ (g) Results: Raw Data Calcium Carbonate Mass of CaCO₃ + Weighing

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    measuring the reactants and products of the reaction. I will also determine the actual yield vs. the theoretical yield by calculating the percent yield. Materials: 1 Distilled water 1 Paper towels 1 Small paper cup 1 Coffee cup or mug 1 Beaker‚ 100 mL‚ glass 1 Funnel 1 Cylinder‚ 25 mL 1 Goggles-Safety 1 Scale-Digital-500g 1 Weighing boat‚ Plastic 1 CaCl2·2 H2O-Calcium Chloride‚ Dihydrate - 2.5 g 1 Filter Paper 12.5-cm 1 NaCO3-Sodium Carbonate - 2 g Procedure 1. Put on your goggles. 2. Weigh out

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    Lab Report

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    BACK TITRATION- DETERMINATION OF THE CARBONATE CONTENT IN GARDEN LIME NAME: OSEI BONSU ERIC ID: 3906409 EXPERIMENT: I.2.2.1.

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    A Paper

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    Lab #16: Gravimetric Analysis of Metal Carbonate Introduction: In this laboratory the identity of group 1 metal Carbonate is determined gravimetrically using a double replacement precipitation reaction. Concepts: Double-Replacement reaction Gravimetric analysis. Background: The identity of group 1 metal M is determined by analyzing an unknown Group 1 metal carbonate‚ M2CO3. There are 3 main reactions in this lab: 1. Equation 1: M­2CO3 (s) → 2M+ (aq) + CO32- (aq) 2. Equation 2: Ca2+

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    quantitative relationships that exist among the reactants and products in chemical reactions To predict the amount of product produced in a precipitation reaction using stoichiometry‚ accurately measure the reactants and products of the reaction‚ determine the actual yield vs. the theoretical yield and to calculate the percent yield. The equation that will be used is: Ba(NO3)2 (aq) + CuSO4 (aq) → BaSO4 (s) + Cu(NO3)2 (aq) Method 1. Gather materials needed for experiment which included:

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    for high school biology students but may be adapted for middle school students. Objectives: The students will be able to describe osmosis and differentiate between the effects of hypotonic‚ hypertonic‚ and isotonic solutions on animal cells and determine the equilibrium point for a chicken egg in corn syrup. They will also be able to apply this knowledge to human colonic (large intestine) epithelium‚ and the effects and consequences hypotonic‚ hypertonic‚ and isotonic solutions would have on these

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    the amount of product that was produced in the precipitation reaction of calcium carbonate by using stoichiometry. Then learn how to figure out the actual yield‚ theoretical yield and percent yield of the experiment. Experiment and Observation: The first step in the experiment was to weigh 1g of CaCl2 +2 H2O‚ then pour it into the 100mL glass beaker with 25mL of distilled water and then stir it to make the solution calcium chloride. The next step was to calculate the amount of Na2CO3 I needed for

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    Hard Water Analysis

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    Na2CO3 → CaCO3 + 2 Na + 2 Cl Purpose: Determine the amount of ions‚ specifically calicum‚ that are present in multiple samples of water by adding another chemical to create a reaction to percipitate the calcium out of the water into a measureable solid Materials: balance (.001g)‚ 100ml beakers‚ graduated cylinder‚ drying oven‚ Na2CO3 (sodium carbonate)‚ stir rod‚ scoopula‚ DI water‚ watch glasses‚ filter paper‚ ring stand‚ funnel‚ water samples with CaCl2 (calcium chloride) Procedure: 1. Measure out

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    be a systemic error due to the calibration of the glassware used in this experiment. A systematic error occurred during this experiment was the inaccuracy of the measuring scale. This is because the same measuring scale was used in each trial to determine the amount of the antacid tablet. However‚ the problem was that there was never one significant value mostly because there is no stable reading. To solve this problem‚ use a more accurate measuring scale to reduce the change in

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    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 up your filtration assembly. After the filtration assembly is ready‚ swirl the contents

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