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9.3 Stoichiometry Mass-Volume Mass- Particles

9.3 Stoichiometry Mass-Volume Mass- Particles. If 70.9 g of Chlorine Gas are used, how many moles of Aluminum Chloride can be produced?. Solving mass-mass problems: Convert the given quantity to MOLES. (Divide mass by gfm)

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9.3 Stoichiometry Mass-Volume Mass- Particles

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  1. 9.3 Stoichiometry Mass-VolumeMass- Particles

  2. If 70.9 g of Chlorine Gas are used, how many moles of Aluminum Chloride can be produced? Solving mass-mass problems: Convert the given quantity to MOLES. (Divide mass by gfm) Calculate unknown moles by multiplying by a mole ratio.(unknown/known) Warm-Up 2 Al + 3 Cl2 2 AlCl3 • What is the mass of the AlCl3 ? 3. Convert the answer in # 2 to mass. (Multiply by gfm)

  3. Other legs of the mole wheel • If given a mass of a reactant you can find # of particles produced • If given the volume (@STP) of a reactant you can find the mass produced • If given the # of molecules of a product you can find # molecules of reactant

  4. 2 H2O2  2 H2O + O2 MnO2 Starting with 29.2 g of hydrogen peroxide How many molecules of Oxygen are produced? What is the volume of the Oxygen gas produced? (assume STP conditions) What mass of water is produced?

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