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Section 3.6: Quantitative Information from Balanced Equations

Section 3.6: Quantitative Information from Balanced Equations. 3.6: Quantitative Information from Balanced Equations.

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Section 3.6: Quantitative Information from Balanced Equations

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  1. Section 3.6:Quantitative Information from Balanced Equations

  2. 3.6:Quantitative Information from Balanced Equations. The coefficients in a balanced equation represent both the relative numbers of molecules involved in the reaction, AND THE RELATIVE NUMBERS OF MOLES, and therefore the relative masses: 2 H2(g) + O2(g) → 2 H2O (l) 2 molecules + 1molecule 2 molecules 2 moles 1 mole 2 moles = 2 x (2.0) g + 32.0 g → 2 x (18.0) g

  3. Weights of products and reactants in a balanced equation: We can thus work out how many grams of water will be produced by burning given amounts of H2 and O2 together. Example: The combustion of butane: 2 C4H10(l) + 13 O2(g) → 8 CO2(g) + 10 H2O(l) 2 moles 13 moles 8 moles 10 moles 2 x 58.0 g 8 x 44.0 g M. Wt. C4H10 M. Wt. CO2

  4. Conversion Sequence Grams Reactant Moles Reactant Moles Product Grams Product

  5. How many grams of CO2 will be obtained by burning 1.00 g of C4H10? 2C4H10 + 13O2 8CO2(g) + 10H2O(g) 1) Grams reactant → Moles reactant 1.00 g x 1mol C4H10 = 0.0172 mol C4H10 58 g C4H10 2) Moles reactant → Moles product 0.0172 mol C4H10 x 8mol CO2 = 0.0688 moles CO2 2 mol C4H10 3) Moles product → Grams product 0.0688 mol x 44.0 g CO2 = 3.03 g CO2 1 mol CO2

  6. Homework • # 3.57-3.60; 3.63-3.64 on pages 114-115

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