used in mothballs‚ produced 8.80g CO2 and 1.44 H2O. Calculate the empirical formula for naphthalene. 8.80g CO2 (find moles of Carbon by dividing the molar mass and doing the molar ratio of C and CO2 = 0.200mol C. 1.44H2O (find moles of Hydrogen by dividing the molar mass of water and doing the ratio of 2moil H/1molH2O) 0.160mol H divide them by the smallest number of moles C = 1.25 H= 1 Multiply 4= 5‚ H=4 1) If the molar mass of naphthalene is 128.18g/mol what is the molecular formula
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vinegar. The second part of the experiment was to see if by titrating a solution of NaOH and an unnamed mystery acid‚ you could find the molar mass of the unknown acid (solving the mystery). It must be understood that the number of moles of the reacting NaOH and the number of moles of the product NaX acid‚ must both equal (in this case 1:1) in order for the calculation to find the molar mass to work. Procedure: Begin the procedure by first making sure all glassware has been cleaned. Next set up the
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figures; • convert physical quantities from one system of units to another; • explain various laws of chemical combination; • appreciate significance of atomic mass‚ average atomic mass‚ molecular mass and formula mass; • describe the terms – mole and molar mass; • calculate the mass per cent of different elements constituting a compound; • determine empirical formula and molecular formula for a compound from the given experimental data; • perform the stoichiometric calculations.
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lab) 1. Use the equations given on the front page to determine the number of moles of sodium thiosulfate that are equivalent to one mole of sodium hypochlorite. 2. From your three trials‚ calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach. 3. Use the average volume and the molarity of Na2S2O3 to determine the molarity of the diluted bleach. (Find moles of Na2S2O3‚ convert to moles of NaClO‚ and divide by volume of dilute bleach that was titrated in each trial
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white crystalline powder with no odor and a bitter taste. It is a derivative of morphine in that the –OH (hydroxyl group) is replaced by an acetyl group‚ -OCOCH3 and has a molecular formula is C21H23NO5 with a molecular weight of 369.42 grams per mole and a melting point of 173°C. Heroin is a schedule I controlled substance meaning it has no medical uses and has a high potential for abuse. Abuse is classified as illegal usage of a drug or excessive use above recommended dosage. Some health effects
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______________________________________________________________________ Combustion Reaction: ______________________________________________________________________ Mole Ratio: ______________________________________________________________________ Diatomic Molecule: ______________________________________________________________________ Mole: ______________________________________________________________________ Hydrocarbon: ______________________________________________________________________
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moles-stoichiometry-practice-problems Now you’re ready to use what you know about conversion factors to solve some stoichiometric problems in chemistry. Almost all stoichiometric problems can be solved in just four simple steps: 1.Balance the equation. 2.Convert units of a given substance to moles. 3.Using the mole ratio‚ calculate the moles of substance yielded by the reaction. 4.Convert moles of wanted substance to desired units. These "simple" steps probably look complicated at first
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1. The mole is a counting unit of chemistry that denotes a specific amount 2. Avogadro created this unit 3. He used 12 grams of carbon to figure out his unit‚ weighed out 12 grams and did multiple test calculations 4. Abbreviation for the mole is mol 5. Avogadro’s number is 6.022 x 10^23 6. 1 mole= 6.022 x 10^23 7. Avogadro used the number to create molar mass 8. Molar mass is the weight of an atom in 1 mol‚ g/mol is the unit 9. MM is the abbreviation for molar mass 10. A mole is defined
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of atoms of an element equal to the number of atoms in exactly 12.0 grams of carbon-12? Mole or Avogadro’s number 5. How many atoms are in a sample of an element whose mass is numerically equal to the atomic mass of that element? 6.02x1023 6. For what substance do we use formula units? Ionic compound 7. At STP‚ equal volumes of different gases contain what? Same number of particles = 1 mole 8. Identify the value for standard temperature. 25C 9. Identify the value for standard pressure
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I. Title: Iron-Copper (II) Chloride Reaction II. Purpose: The purpose of this lab is to see how iron reacts with a copper (II) chloride solution. III. Equipment and Reagents Scoop copper (II) chloride (CuCl2) Beaker Iron (Fe) Wash Bottle water (H2O) Scale Hydrogen chloride (M HCl) Filter Paper IV. Procedure: 1. Obtain a clean‚ dry 250 mL beaker. 2. See teacher to obtain a scoop of CuCl2 in the beaker. 3. Add approximately 50 mL of tap water to
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