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Stoichiometry

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Published in: Chemistry
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This PowerPoint presentation focuses on stoichiometry, the branch of chemistry that deals with the calculation of reactants and products in chemical reactions. Stoichiometry is essential for understanding the quantitative relationships in chemical reactions and is foundational for laboratory work, industrial processes, and environmental science. This presentation is designed for high school and introductory college students, providing a comprehensive understanding of stoichiometry and its crucial role in chemistry.

Mudasir A / Jammu

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  1. Stoichiometry "In solving a problem of this sort, the grand thing is to be able to reason backward. This is a very useful accomplishment. and a very easy one, but people do not practice it much." Sherlock Holmes, in Sir Arthur Conan Doyle's A Study in Scarlet Stoichiometry The study of quantities of materials consumed and produced in chemical reactions.
  2. CA Standards Stu ents now ow to describe c emica reactions by writing balanced equations. Stu ents now t e quantity one moe is set by e ining one moe of carbon 12 atoms to have a mass of exactly 12 grams. Stu ents now one mo e equa s 6.02 10 3 partic es atoms or molecules). Students now ow to determine t e mo ar mass o a mo ecu e from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure. Stu ents now ow to ca cu ate t e masses o reactants an products in a chemical reaction from the mass of one of the reactants or products and the relevant atomic masses.
  3. Calculatinq Masses of Reactants and Products Balance the equation. 1. 2. Convert mass or volume to moles. if necessary. 3. Set up mole ratios. 4. Use mole ratios to calculate moles of desired substituent. 5. Convert moles to mass or volume. if necessary.
  4. Working a Stoichiometry Problem 6.50 grams of aluminum reacts with an excess of oxygen. How many grams of aluminum oxide are formed. 1. Identify reactants and products and write the balanced equation. 4 Al + 302 2 A1203 a. b. c. d. Every reaction needs a yield sign! What are the reactants? What are the products? What are the balanced coefficients?
  5. Working a Stoichiometry Problem 6.50 grams of aluminum reacts with an excess of oxygen. How many grams of aluminum oxide are formed? 3 02 6.50 x 2 x 101.96 * 26.98 6.509.4 1 2 26.989.4 4 2A1203 — 4 = 12.3 g A1203 101.96 g A1203 1 mp1--Äi203
  6. Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature and pressure, then mole ratios of gases are also volume ratios. 3 H2(g) moles 1-42 3 3 liters 1-42 N2(g) + 1 mole N2 1 liter N2 -5 2NH3(g) moles NH 3 2 2 liters NH 3
  7. Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters of hydrogen react with an excess of nitrogen? H2(g) + N2(g) _2NH3(g) 3 12 2 L NH3 8.0 L NH3
  8. Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2 KC103(s) 2 KCl(s) + 3 02(g) 50.0 g-.wf03 1 mol-KC103 122.55 g._KCi03 3 mol-02 22.4 L 02 2 mol-KC103 1 mol-Ö2 13.7 LO 2
  9. Gas Stoichiometry #4 How many liters of oxygen gas, at 37.00C and 0.930 atmospheres, can be collected from the complete decomposition of 50.0 grams of potassium chlorate? 2 KC103(s) 2 KCl(s) + 3 02@) 50.0 g.-wf03 nRT p 1 mgVKC103 122.55 g.-KCj03 3 mol 02 2 mol-KC103 L •atm mol •K 0.930atm 0.612 mol 02 16.7 L

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