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Stoichiometry: Mole Ratios & Equations Balancing for Chemical Reactions

Learn how to calculate mole ratios and balance chemical equations with stoichiometry in this insightful guide. Understand the roots, interpretations, and examples for successful chemistry studies.

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Stoichiometry: Mole Ratios & Equations Balancing for Chemical Reactions

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  1. Do Now In order to make 1 salad it requires 1 head of lettuce, two tomatoes and three carrots. What would be the coefficients for the lettuce, tomatoes, and carrots assuming you wanted to make 3 salads? Write the coefficients below! In order to make 1 bike it requires 1 horn, 2 tires, and 1 chain. What would be the coefficients for the horn, tire, and chain, assuming you wanted to make 4 bikes? Write the coefficients below! In order to make 1 batch of cookies it requires 2 cups flour, 3 eggs, and 1 cup sugar. What would be the coefficients for the flour, eggs, and sugar, assuming you wanted to make 10 batches of cookies? Write the coefficients below! 3 4 10

  2. Day 1 - Notes Unit: Stoichiometry Using Mole Ratios and Review of Balancing Chemical Equations

  3. After today you will be able to… • Calculate the number of moles of a substance that can be produced from their coefficients in the balanced chemical equation • Review of the basics of how to balance a chemical equation

  4. The wordstoichiometrycomes from the Greek words: stoicheion(meaning "element") metron(meaning "measure") Stoichiometry: The study of quantities as it relates to chemical reactions. Based on the roots, what does it mean?

  5. Balanced chemical equations can be interpreted many ways… 1. Molecules • 1N2(g) + 3H2(g) 2NH3(g) H • molecules: N N H H H H H H H H H H N N +  H

  6. Balanced chemical equations can be interpreted many ways… 2. Mass • 1N2(g) + 3H2(g) 2NH3(g) • (6 x 1.01) • (2 x 14.01) • (6 x 1.01) + (2 x 14.01) +  • 34.08g • 28.02g • 6.06g • 34.08g • = • 34.08g • Mass of reactants and products are always equal!

  7. Balanced chemical equations can be interpreted many ways… 3. Mole Ratio • 1N2(g) + 3H2(g) 2NH3(g) • moles: +  • 2 mol NH3 • 1 mol N2 • 3 mol H2 • This is the relationship we will focus on in this unit!

  8. Mole-Mole Calculations • The coefficients in the balanced equation represent the smallest whole number mole ratio between reactants and products.

  9. Mole-Mole Calculations • Examples of mole ratios for the reaction: • 1N2(g) + 3H2(g) 2NH3(g) 1 mol N2 2 mol NH3 3 mol H2 1 mol N2 2 mol NH3 3 mol H2

  10. Mole-Mole Calculations • Example: If 3.86 moles of potassium reacts completely with excess water, how many moles of hydrogen would be produced? hydrogen hydroxide water potassium +  potassium hydroxide + hydrogen __K 2 __ H(OH) 2 __ K(OH) + __ H2 1 2  + K: 3.86 mol K U: ? mol H2 3.86 mol K 1 1 mol H2 2 mol K 1.93 mol H2 x =

  11. Mole-Mole Calculations • Example: How many moles of aluminum will react with 0.512 moles of hydrochloric acid? hydrogen chloride aluminum + hydrogen chloride aluminum + hydrochloric acid  __Al 2 __HCl 6 __ AlCl3 + __ H2 3 2  + K: 0.512 mol HCl U: ? mol Al 2 mol Al 6 mol HCl 0.512 mol HCl 1 0.171 mol Al x =

  12. Questions? Begin HW1

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