Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 81b

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Chapter 3, Problem 81b

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of silver carbonate are present after the reaction is complete?

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Write the balanced chemical equation for the reaction between sodium carbonate (Na2CO3) and silver nitrate (AgNO3) to form silver carbonate (Ag2CO3) and sodium nitrate (NaNO3).

Calculate the molar mass of sodium carbonate (Na2CO3) and silver nitrate (AgNO3) to convert the given masses from grams to moles.

Using the stoichiometry of the balanced equation, determine the limiting reactant by comparing the mole ratio of sodium carbonate to silver nitrate.

Calculate the theoretical yield of silver carbonate (Ag2CO3) by using the moles of the limiting reactant and the stoichiometry of the reaction.

Convert the moles of silver carbonate formed to grams using its molar mass to find the mass of silver carbonate produced in the reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the proportions of substances involved in a reaction, which is essential for predicting the amounts of products formed from given quantities of reactants.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, enabling the calculation of how much of a product can be formed from a specific amount of reactant in a chemical reaction.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble solid, known as a precipitate. Understanding these reactions is important for predicting the formation of products, such as silver carbonate in this case, and determining the quantities of reactants consumed and products formed.

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Textbook Question

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

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Textbook Question

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH₃ to NO: 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) In a certain experiment, 2.00 g of NH₃ reacts with 2.50 g of O₂. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

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Textbook Question

Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid and grams of acetic acid present in the mixture after the reaction is complete.

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Textbook Question

Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of lead(II) acetate present in the mixture after the reaction is complete.

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Textbook Question

When benzene 1C6H62 reacts with bromine 1Br22, bromobenzene 1C6H5Br2 is obtained: C6H6 + Br2¡C6H5Br + HBr (a) When 30.0 g of benzene reacts with 65.0 g of bromine, what is the theoretical yield of bromobenzene?

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