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Understanding Chemical Reactions: Reactants, Products, and Stoichiometry

Chemical reactions are represented by formulas showing reactants and products, which can be in different states: aqueous (aq), gas (g), liquid (l), or solid (s). It's crucial to balance these reactions in accordance with the law of conservation of matter, meaning mass cannot be created or destroyed. Coefficients of reactants and products provide molar ratios essential for calculations in stoichiometry. This guide explores balancing reactions, calculating moles and masses, and understanding the implications of coefficients with practical examples.

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Understanding Chemical Reactions: Reactants, Products, and Stoichiometry

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  1. Chemical Reactions

  2. Representing a Chemical Reaction: A chemical reaction is always represented in a certain way : At the start of a reaction At the end of a reaction we have we have ReactantsProducts HCl (aq) + Ca(OH)2(s) CaCl2(aq) + 2 H2O (l) The reactants and products can be in various states, and it is important to note if they are aqueous ,(aq),gas, (g), liquid, (l), or solid ,(s).

  3. Law of Conservation of Matter:Balancing Chemical Reactions Matter cannot be created nor destroyed. • The total mass of the reactants in a chemical reaction must be equal to the total mass of the products formed. • The coefficients in a chemical reaction must always be balanced in order to ensure that there are an equal number of each atom on both “sides” of the reaction.

  4. Examples: • Place the correct coefficient in each blank space in order to balance the following reactions: __ MgF2 + __ K  __ KF + __ Mg __ H2 + __ O2  __ H2O __ Al + ___ O2  ___Al2O3

  5. ** EST Molar Ratios & Stoichiometry The coefficients in a chemical reaction are very important. They give us the molar ratioin which the substances react and form. 1HCl (aq) + 1Ca(OH)2(s) 1CaCl2(aq) + 2 H2O (l) In the above example, the coefficients show that when 1 mole of HCl reacts with 1 mole of Ca(OH)2 there will always be 1 mole of CaCl2and 2 moles of H2O formed.

  6. We can use the molar ratios to determine the quantity (mass or moles) of reactants or products in a chemmical reaction. Any calculation that uses the molar ratio is a stoichiometric calculation.

  7. Example: 2HCl (aq) + 1Ca(OH)2(s) 1CaCl2(aq) + 2 H2O (l) • Using the molar ratio, how many moles of H2O would form if 6 moles of HCl react with 3 moles of calcium hydroxide? • How many moles of calcium chloride are formed when 180 grams of water if formed?

  8. 1HCl (aq) + 1Ca(OH)2(s) 1CaCl2(aq) + 2 H2O (l)

  9. Ex. What mass of oxygen is required to produce 4.4 grams of carbon dioxide, CO2? C2H4 (g) + 3O2 (g)  2CO2 (g) + 2H2O (l) 4.8 g 4.4 g 44 g/mol 32 g/mol 0.15 mol 0.1 mol

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