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Stoichiometry Lab Report

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Example Problem Stoichiometry 4NH3(g) + 6NO(g)→5N2(g) + 6H2O(g) How many moles of each reactant were there if 13.7 moles of N2(g) is produced? ×4 moles NH3(g) = 10.96 moles NH3(g) ×6 moles NO(g) = 16.44 moles NO(g) So we have 10.96 moles NH3(g) and 16.44 moles NO(g). Problem: What is the mass of 2 moles of H2S ? GFM of H = 1 GFM of S = 32>br> GFM of H2S = 2×1 + 32 = 34 grams / mole ×34 grams = 68 grams Percentage Composition by Mass H2O One mole of water is 18.0152 grams. In that compound, there are two moles of H atoms and 2 x 1.008 = 2.016 grams. That's how many grams of hydrogen are present in one mole of water. There is also one mole of oxygen atoms weighing 16.00 grams in the mole of water. To get the percentage of hydrogen, divide the 2.016 by 18.015 and multiply by 100, giving 11.19%. …show more content…

Empirical Formula and Molecular Formula Caffeine has an elemental analysis of 49.48% carbon, 5.190% hydrogen, 16.47% oxygen, and 28.85% nitrogen. It has a molar mass of 194.19 g/mol. What is the molecular formula of caffeine? 49.48% C, 5.190%H, 16.47% O and 28.85% N Step 1 Assume a mass of 100g so % becomes

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Eventually using the NaOH and the acid’s consumed moles, the equivalent mass will be determined. Procedure: Part 2: Obtain 45mL of NaOH, and then weigh 0.3-0.4g of the unknown acid (KH2PO4). Dissolve the acid into 20.00mL water.

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Green with a silver nitrate (AgNO3) solution. Assuming that certain amounts of AgNO3 was dissolved in a particular amount of water to produce the solution. Find out how many moles of Na2CO3 were involved in the silver nitrate reaction first. To my knowledge of Mr. Green’s addition of 1.5 grams of Na2CO3 to the silver nitrate solution comes from the statement. Since Na2CO3 has a molar mass of 105.99 g/mol, the amount of Na2CO3 is: moles of Na2CO3 = mass / molar mass moles of Na2CO3 = 1.5 g / 105.99 g/mol moles of Na2CO3 = 0.0141 mol

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75.33 grams Weight of the unknown = 0.23 grams Calculation : 75.33-75.10/0.36x100 = 63.8 % recovery Melting point of

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Which was 117.60 grams for substance 1, 87.71 grams for substance 2, 54.7 grams for substance 3, 25.11 grams for substance 4. Once we finished weighing each unknown substance we started figuring out the g/mol mass of each compound that the substances could possibly be, which is how we got to Table #2 above. In order to find the g/mol mass of each of the compounds, we had to find the molar mass of each element, then multiply and add accordingly. I'll use K2SO4 as an example of how to calculate the molar mass of a compound. The elements in K2SO4 are Potassium, Sulfur, and Oxygen.

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What is the molecular formula if the molecular weight is 58.0 g/mole? A compound containing Sulfur and Nitrogen is 69.6% Sulfur by mass. If its molar mass is 184 g/mole: What is the empirical formula What is the

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Percentage Composition of Hydrates The Introduction: Hydrates are ionic compounds and are often a type of salt with a definite amount of water as part of their structure. Hydrates are decomposed into anhydrous salt, a no-water compound, and water vapor when heat is applied; water vapor is released from the hydrated compound, which leaves with an anhydrous salt that weighs less than the hydrate. But how do we find the percent of the water that was lost after applying heat to the hydrates and how accurate is finding the percent composition of water using experimentation and a gram weight scale? The purpose of the experiment is to find the percent of water lost by finding the difference between the mass of hydrate and the mass of anhydrous

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Stoichiometry is a method used in chemistry that involves using relationships between reactants and products in a chemical reaction, to determine a desired quantitative data. The purpose of the lab was to devise a method to determine the percent composition of NaHCO3 in an unknown mixture of compounds NaHCO3 and Na2CO. Heating the mixture of these two compounds will cause a decomposition reaction. Solid NaHCO3 chemically decomposes into gaseous carbon dioxide and water, via the following reaction: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g). The decomposition reaction was performed in a crucible and heated with a Bunsen burner.

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Which of the following unit is used to indicate mass? a. Cm3 b. Um c. Mg d. mL 21. Which of the following demonstrate a chemical reaction of water?

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This means that the mass of the anhydrous, AlK(SO4)2, was 0.75g and the water driven off was 0.68g. When my lab partners and I used these measurements for our calculations we got the ratio of 1:13. This ration is clearly accurate because the actual ration is

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x Volume of KMnO4 = mol MnO4- 0.025 M x 15.31mL x (1 L/ 1000 mL) = 3.83 x 10-4 mol MnO4- Determining mol H2O2 mol MnO4- x [ 5 mol H2O2 / 2 mol MnO4- ]= mol H2O2 3.83 x 10-4 mol MnO4- x [ 5 mol H2O2 / 2 mol MnO4- ] = 9.57 x 10-4 mol H2O2 Determining mass of H2O2 mol H2O2 x Molar Mass of H2O2 = mass of H2O2 9.57 x 10-4 mol H2O2 x 34.016 g/mol = 0.0326 g H2O2 Determining the volume of H2O2 mass of H2O2 x Density of H2O2 = volume of H2O2 0.0326 g/mol x 1.00 L/g = 0.0326 L H2O2 Determining the percent composition of H2O2: (volume of solute / volume of solution)

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Ideally, every mole of each reagent would be used up, and theoretical yield, we are assuming that every last mole of the reactants would

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Empirical Formula of Magnesium Oxide - Lab Report Background Information/Introduction: The aim of this lab is to determine the empirical formula of magnesium oxide by converting magnesium to magnesium oxide. As an alkali earth metal, magnesium reacts violently when heated with oxygen to produce magnesium oxide and magnesium nitride as a byproduct. In order to obtain only magnesium oxide, distilled water was added so that magnesium nitride will react and convert to magnesium hydroxide. Further heating then oxidizes all of the magnesium into magnesium oxide.

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You can determine this by calculating the mass and moles of H20 driven off. 3. The formula is

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Mole ratio is considered a conversion factor since it helps to convert units with the use of moles. It is used in stoichiometry and other calculations and comes out of the balanced chemical equations. Stoichiometry is the measurement of elements that concerns the chemical quantities produced or taken in a reaction. The process of relating the mass and mole quantities of reactants or products in a reaction. It uses a balanced chemical equation, mole ratio, and sometimes needs mole mass.

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One mole of anything equals 6.022 x 1023, also known as Avogadro’s number. The mass of one mole can be determined by Molar mass= 1

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